Bifunctional Ligands Discerning and Medicinal Chemistry of ... · Bifunctional Ligands in...
Transcript of Bifunctional Ligands Discerning and Medicinal Chemistry of ... · Bifunctional Ligands in...
Bifunctional Ligands in Discerning and Developing the Fundamental
and Medicinal Chemistry of B i s m u t h o
Glen G. Briand
Submitted in partial filfiliment of the requirrments
for the degree of Doctor of Philosophy
Dalhousie University
Halifax, Nova Scotia
Juiy 1999
@ Copyright by Glen G. Briand, 1999
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For Janice
Table of Contents
Table of Contents ...................................................................................... v
List of Figures ........................................................................................... ix
List of Tables .......................................................................................... x
Abstract ................................................................................................... xii
... ............................................................. List of Abbreviations aad Symbols xiii
Acknowledgrnents ......................................................................... xvii
. ......................................................................... Chapter 1 Introduction 1
1 . 1 Bifunctional Ligands as a Means to Denning the Coordination
Chemistry of Bismuth ............................................................... 1
1.2 Structurai Divmity in Bismuth Chemistry ....................................... 5
1 . 3 Characterization Techniques ......................................................... 6
.......................................... 1.4 Scope of Thesis and General Comments 8
1.5 Conclusions . Industry and the Scientific Method ............................... 9
Chapter 2 . The Chemistry of Medicina1 Bismuth Compounds: Hydroxy-/
Alkoxycarbox ylates and Inorganic Salts .................................................... 12
Introduction .......................................................................... 12
Inorganic Compounds ........................................................... 13
Carboxylates and Dexivatives ....................................................... 20
2 . 3 . Poiyhydroxycarboayfic Acid Complexes ............................... 20
................... 2.3.2 PoIyuminocarboxyJates and ~ioIatoc(~rboxyJutes 26
2.4 'ColloidaI Bismuth Subcitrate' (CBS). 'Bismuth Subsalicylate' (BSS)
and 'Ranitidine Bismuth Citrate' (RBC) ................................................ 27
2.5 Models and Alternatives for Bioactive Bismuth Compounds ................ 32
2.6 Interactions with Biomolecules and Phmaceutical Agents .................. 35
2.7
Chapter 3 .
3.3
3.4
Chapter 4 .
................................................................ 2.6.2 Amino Aci'ds 35
...................................................... 2.6.2 Pqptides und Proteins 36
2.6.3 Xnzeruc~ion of Bismuth Compun& witA Other Dmgs and
............................................................... Food Camponents 38
................................................................... 2.6.4 Antidotes 39
Conclusions ........................................................................... 40
Toward the General Synthesis of Dicarboxylates and the Structural
Characterization of Bismuth Oxdate .................................. .., .................. 42
Introduction .............................................................................. 42
Synthesis and Structure of Bismuth Carboxylates ................................... 43
............................................................... 3.2. I Carhxylates 45
.............................................................. 3.2.2 DicnrbaxyIates 49
................................................................ Results and Discussion 51
................................................. Conclusions and Future Directions 54
Aminocarboxylates: New Investigations into the Bi- System
.................................. Including Isolation of the First CatioNc Complex 58
Introduction ............................................................................. 58
......................... S ynthesis and Structure of Bismuth-Aniin&xy lates 58
............................................................... Results and Discussion 69
.......................................................... 4.3.1 Synthetic Shrdies 69
4.3.2 Prefiminary Electrosproy Mass Spectrometry Snidies of the
...................................................................................... Bi-&fa System 74
................................................. 4.4 Conclusions and Future Directions 75
......................................... Chapter 5 . Introduction to Bismuth Thiolate Chcmistry 78
........................................................................... 5.1 Introduction 78
......................................................................... 5.2 Monothiolates 78
............................................................... 5.3 Bifiinctional Thiolates 84
.................................................................. 5.3.1 Dithiolates 84
5.3.2 TIriuiatocarboxylates ...................................................... 89
..................................... 5.3.3 Hydroxy-/Alkoxy- and Ketothiolates 91
....................................... 5.3.4 Amino-, Imino- and Ara-Thiolates 95
....................................................... 5.4 Thio- and Dithiocarboxylates 101
.......................................................... 5.4.1 ThiocarboxyIates 102
5.4.2 Dithiocarboqdates (Dithiocarbamates. Dithioxanthates) ......... 103
.......................................................... 5.5 Summary and Conclusions 113
Chapter 6 . Definhg and Controlling the Arninoethanethiolate Chemistry of
Bismuth(III): Synthesis and Comprehemive Characterization of
..................................................... Homologous Thiolatobismutth Series 116
.......................................................................... 6.1 Introduction 116
............................................................. 6.2 Results and Discussion 118
.............................................. 6.3 Conclusions and Future Directions 130
Chapter 7 . (Methy1estei)methanethiolates: The First Ester Complexes of
Bismuîh(m) as a Step Toward Modeling 'Colloidal Bismuth
Subcitrate' ............................................................................................. 135
7.1 Introduction .................................................................... 135
7.2 Synthesis and Structure of Bismuth-Organocarbonyl Complexes .......... 135
7.3 Secondary Bonding and the tram ERect: the Role of a* Orbitals .......... 139
7.4 Results and Discussion ........................................................ 140
7.5 Conclusions and Future Direction ................................................. 147
Chapter 8 . Experimental ...................................................................... 151
8.1 General Procedures ................................................................... 151
8.2 Synthetic Procedures ............................................................... 151
8.3 Physical and Spectroscopie Data .................................................................... -160
8.4 X-ray Cxystallogcaphic Data ...................................................................... 168
References .......................................................................................... -173
viii
List of Figures
Figure 1.1 Bismuth bonding arrangements witb organic functional groups and their
heavier group 1 5 and 16 analogues ........................................................ 2
Figure 1.2 Bifunctional combinations for developing the chemistry of bismuth .......... 4
Figure 1.3 APCI-mass spectnun of bis(hydroxethane~olato)bi~~nuth(III) nitrate
550 in acetonitrile ............. .........-.... .......................-.....-................................. 7
Figure 3.1 Crystallographic view o f Di(C@,), 1, 0 8H20 38 .................................. 52
Figure 4.1 Crystallographic view of {[Bi(&&)], H} CI.2H20 ....................... 70
Figure 5.1 Bonding situations observeci for bismuth thiolate complexes .................... 114
Figure 6.1 Crystallographic view of Bi(SCH2CH2N&)3 hq .............................. 124
Figure 6.2 Crystallographic view of Bi(SCH2CH2NHJ2Cl =CI ......................... 125
Figure 6.3 Crystailographic view o f Bi(SCH2CH2NMe3, Cl 68(Me)C1 ................. 126
Figure 6.4 Crystallographic view o f the tetramer of Bi(SCH2CH2NMeC12
6C(Me)WiHCl 127 - ........................................
Figure 6.5 Crystailographic view of Bi(SCH2CH2NHMGC13 m(Me)CI .............. 128
Figure 6.6 Crystallographic view of Sb(SCH2CH2N&)C1 a C I .......................... 131
Figure 7.1 Crystailographic view of polymenc arrangement of
Pi(SCH,COOCH, )2Cl] ............................................................. 142
Figure 7.2 Crystallographic view of the dimeric arrangement of
[si(SCH2C0OCHJ3 ] ................................................................. 143
Figure 7.3 Crystdlographic view of the polymcric arrangement of
K p i {SCH(CH,)COO} C1J Iç .......................................................... 1 46
List of Tables
Table 2.1 Compound designatioas and assigned formulae for medicinal inorganic
........................................................................ bismuth compouads 14
Table 2.2 Characterization data for isolated bismuth hydroxy-/alkoxycarboxylates ... - 2 1
Table 2.3 X-ray crystallographic data for solids descnbed as colloidal bismuth
subcitrate .............................................................................................................. 30
................................. Table 2.4 Exarnples of other bioactive bismuth compounds 34
Table 3.1 Analytical data for carboxylate and dicarboxylate compounds ................... 44
................................. Table 4.1 Anaiytical &ta for aminocarboxylate compounds 59
............................... Table 4.2 Selected bond lengths for [ (Bi-Hm] complexes 73
...................................... Table 5.1 Analytical data for monothiolate compounds 79
........................................... Table 5.2 Analytical data for dithiolate compounds 84
Table 5.3 Analytical &ta for thiolatocarboxylate compounds ............................... 89
Table 5.4 Analytical data for hydroxy-/dkoxy- and ketothiolates ........................... 92
Table 5.5 Analytical data for amino-. irnino- and azathiolate compounds ................... 96
.................................. Table 5.6 Analytical data for tbiocarboxylate compounds 102
............................... Table 5.7 Anaiytical &ta for dithiocarboxylate compounb 104
......................... Table 6.1 Selected bond distances (A) for aminoethanethiolates 123
......................................... Table 7.1 Andytical data for carbonyl compouuds 1 36
Table 7.2 Comparimn of selected bond lengths (A) in bismuth-esterthiolate
................................................................... and related complexes 144
........ Table 8.1 Reaction conditions and isolation conditions for thiolate complexes 154
Table 8.2 Yields and elcmcntai analyses for al1 compoimds .................................... 158
Table 8.3 Complete vibrational chta for ail compounds ..................................... 160
Table 8.4 Melting points. prominent APCI-MS peaks. and 'H and "C NMR
Data for d l compounds ....................................................................... 164
Table 8.5 Peak assignments of the APCI mass spectra of
bis(hydroxyethanethio1ato)-bismuth salts [Bi(SCH,CH2 0 H ) A ................... 166
Table 8.6 MS/MS assignments for bi~ydr0xyethanCthiolato)bismuth~
saits Pi(SCH,C& OHXX] ................................................................ 167
Table 8.7 Crystailographic data for al1 complexes ........................................... 168
The serendipitous discovery and pharmaceuticd use of bismuth compounds,
dong with fùndamental interests, ha9 prompteci a cenhiry of chernical and clinical studies
of bismuth complexes and prepatations. The characteristic hydrolytic instability and
polymenc nature of these materials has detmed comprehensive chemical studies. As a
result, the chemistry of bismuth, as for many elements of the paioCic table, m a i n s in its
infancy. This work establishes the utility of bifùnctional ligands as a method to
overcoming these obstacles, and represents significant developments in the thiolate and
carboxylate chemistry of bismuth, the latter of which encompasses phamiaceutical
implications. The synthetic guidelines outlined are Wrely to be generally applicable to
other metals and various bifùnctionai ligand combinations.
List of Abbreviations
1 8-crown-6
APCI
avg .
bio.
bivv
br
BSC
BSN
BSS
calc
CBS
Ch
CI
ccord
conc.
con
cry s
cv
1,4,6,10,13,16-
hexaoxacyclooctadecane
atrnospheric pressure
chemicai ionization
average
biological
bip yridine
broad
bismuth subcarbonate
bismuth subnitrate
bismuth subsalicylate
calculated
colloidal bismuth
subcitrate
chalcogen
chemical ionization
coordination
concentrated
conduc tivi ty
crystals
cyclic voltammetry
c ysteine
decomposition point
dip yridine
Na-dimethy l fomamide
Na'-dimethylpropy lene-
urea
dimethylsulfoxide
dipivaloylmethanate
différentia1 thermai
analy sis
dithiocarbamate
dithioxanthate
p o l ~ g r a p h ~
elemental analysis
electnon impact ionization
electrospray ionization
Fourier transforrn
glutathione
glutaric acid
glycine
2-mercaptopropionic acid
Ha3mpa
H U
Hacac
H,bal
Hbdrnap
Hd-
H,cit
H,cvs
H,cvdta
H4cvdtpa
H,dapts
Hm
H&a
wz
Heacd
3-mercaptopropionic acid
aminobenzenethiol
acetylacetone
British anti-Lewisite
1,3-bis(dimethylamh0)-2-
propanol
4,s-benu>br,polone
citric acid
cysteine
zrans-c yclohexane- 12-
diaminetetraacetic acid
N- (2-aminoethyl)-tr~m-
1 2-diarninocyclohexane-
N-NW * *-pentaacetic acid
26-diacetylp yridine
bis(thiosemicarbazone
dirnethoxybenzenethiol
diethylenetriarninepenta-
acetic acid
3-mercapto- 1,s-
diphenylformazan.
dithizone
2-a~ninocyclopcnt- l -cm-
1-dithiocarboxylic acid
eth ylenediamintetraacetic
acid
ethyhaitolate
gallic acid
lactic acid
nitrilotriacetic acid
malic acid
2-methyl-8-
mercaptoquinolinol
maleonitriledithiol,
dicyanoethylene-
1,2-dithiolate
methionine
hexarnethylphosphor-
amide
N-hydroxyethyl-
ethylenediaminetetra-
acetic acid
Hm-hydroxyethyl-
nitnlodiacetic acid
Htnrr oxaiic acid
hTF
H,tar
H m
H,tsal
'Pr
IR
m
M'
Me
med.
mP
MS
pyridinee2,6-dicatboxylic
acid
D-(-)-penicillamine
phthalic acid
2-phenyl-8-
mercaptoquinolinol
quinaldic acid
salicylic acid
thiosernicarbazone
triethylenetriaminehexa-
acetic acid
human serurn transferrin
tartaric acdi
thioglycolic acid
thiosalicylic acid
isopmpyl
infrared
medium
molecular ion
methyl
medicinal
melting point
mass spectrometry
MT
MTP
M W
m/z
NMR
P m *
Ph
dEn
Pot
PP*
PreP
OY
Ram
pwdr
RBC
re f
tel.
RMBP
tandem mass
metallothioneh
metallothionein-Iike
proteins
molecular weigfit
mas-to-charge ratio
nuclear magnetic
resonance
paramet ers
phenyl
1,l O-phenanthroline
potentiometry
parts per million
preparation
Raman spectroscopy
ranitidine bismuth citrate
re ference
relative
S
sh
sol
sp
t
'Bu
TGA
thf -
singlet (strong w.r.t. IR
and Raman)
shoulder
solubiiity
sublimation point
triplet
tertiary butyl
thennogravimetric
analysis
tetrahydro fùran
tetramcethylsilane
tbiosemicarbazide
thiourea
ultraviolet-visible
spectroscopy
volts
very strong
weak
X-ray di fit tion studies
xvi
Firstly, I would like to thank my fiance Janice for her patience, understanding
and support, as well as our families for encouragement during both of our academic
careers.
A huge thank you goes out to Neil Burford for his optimism and motivation,
"profuse" promotion, camaraderie, and most importantly, for teaching me what it means
to be a scientist. "Press on, Neil!"
Gratitude is also extended to our collaborator Dr. T. Stan Cameron for sharing his
crystallographic expertise and being very accommodatïng over the past four years.
A special thanks to the past and present members of the Burford group for al1 their
assistance and discussions: Dr. Lisa Agocs for showing me the ropes; G. Bradley Yhard
for mass spectrometry instruction; Hamilton Maguire; Dr. Charles L.B. Macdonald and
Andrew Phillips for experimental aid; Dr. Daren Leblanc for crystallographic assistance;
Donna Silvert and Luke Y.C. Chen for experimental contributions; T. Danny Lawen and
Arthur House for reference management; and Denise Walsh for conversation.
1 would like to acknowleâge Drs. L. Rnmaley and J.S. Grossert, Brent Jewett,
Beata Kolakowski and Larry Campbell for mass spectrometry support and the Dalhousie
Mass Spectrornetry Centre for use of facilities; Drs. D. Hwper and M. Lumsden and the
ARMRC; Dr. K. Grundy for sitting on my cornmittee; Dr. RJ. Boyd for his suppon; and
Drs. W. Kwiatkowski and H. Jenkins for crystallographic assistance.
Thanks to our collaborators in microbiology and gastroentemlogy, Drs. D.
Mahony, P. Hof3tmaun, and S.J.O.V. van Zanten, L. Bryden and S. Lim-Momson, for
helpful discussions.
Many thanks to al1 of the fnends 1 have made during m y t h e at Da1 for making
my stay very enjoyable.
Finally, 1 would like to thank Dalhousie University, the Walter C. Sumner
foundation, MDS Sciex and Daihousie University for huidiag my meaifh
Chapter 1. Introduction
1.1 Bifunctiond Ligands as a Means to Definhg the Coordination Chemistry of
Bismuth
In light of the potential bioactivity of bismuth cornpounds, the prelude to this
project '" involvecl the synthesis of series of bismuth thiolate cornpoumis as simple
rnodels for complex commercial phamaccutical bismutth materials. A variation in
antimicrobial bioactivity among series members suggests a stnicture/activity relationship
for the bismuth environment,' highlighting the need for univenally applicable synthetic
procedures to control the coordination chemistry of bismuth. Further, the comprehensive
structural and spectroscopic characterization of systematic series of compounds
represents the most reliable fundamental foundation for rational chernical development.
This work represents significant advances in the thiolate chemistry of bismuth, a
movement toward development of generai procedures for preparing and studying the
chemisûy of bismuth carboxylates, and illusation of the role of secondary fitnctional
groups in bridging the gap between these areas. These goals have been achieved through
the preparative, spectroscopic and structural study of compounûs containbg bismuth
complexed with hydrocarbon ligands bearing two (bifùnctional) or more (polyfunctional)
donor sites, as shown in Figure 1.1.
Bifunctional ligands are excellent tools for probing the fiindamental and
biological chemistry of bismuth for various rca~011~. Firstly, they provide simplet models
of organic polyfunctional ligands, which are components of mcdicinal compounds such
\ Ch-Bi
O alkoxide S thiolate Se selemolate
-A Ch-Bi
ketone thione
0,0 carboxylate 0,s thiocarboxylate S,S dithiocarboxylate
organic amide
N amide
ester
amine phosphine arsint
Figure 1.1 Bismuth bonding anangemmts with organic fûnctional groups and their heavia group I 5 and 16 anaIogues.
3 as 'colloidal bismuth subcitrate' (citrate) and 'bismuth subsalicylate' (salicylate).
Secondly, introduction of the thiolate moiety stabilizcs components with respect to
hydrolysis and the precipitation of basic bismuth salts in aqueous media under various pH
conditions. Subsequently, this allows for the study of the interaction of the bismuth
center with other biological and organic hctional groups, and gives a greata
undentandhg of the role of bismuth in biological systems. Discussions in this thesis,
therefore, focus primarily on the chemistry of bismuth cornpouods containing the ligand
or ligand bgrnents show in Figure 1.2. These ligands facilitate the formation of five-
membered rings which have proven to be the most favourabk structural arrangement for
chelate complexes of Systematic alteration of one functionality imposes subtle
changes on the chemistry of bismuth. Ten of these bifiinctional combinations have been
studied to some degne in the literature or as part of this project and are discussed in this
thesis (designated by *).
B y emplo ying these bi fûnctional ligands, this thesis out lines some general and
important observations concerning the significance of chelate ability and pH in the
isolation of bismuth dicarboxylates (Chapter 3) and aminocarboxylates (Chapters 4) in
aqueous media. Similarly, control of the Lewis acidity and thiolation of bismuth are
explored (Chapter 6). and simple models for CBS and other bismuth complexes in
biologicai systems are developed (Chapter 7). Also provided as an introduction to these
topics is the preparation, structure and aqueous chcmishy of commercial bismuth
products and bismuth chemistry relevant to biologicai and medicinal activity (Chapter 2),
as well as the pnparation and structure of established bismuth thiolate compounds
Figure 1.2 Bihuictional combinations for developing the chemistry of bismuth. Designated compounds (*) have bccn used as rcagmts with bismuth, as discussed in this thesis.
5 (Chapter 5). Structurai studies demonstrate a variety of bonding situations which are the
basis for the rnajority of discussions in this thesis.
1.2 Structural Diversity in Bismutb Chemistry
As a main group heavy metal, compounds of bismuth exhibit immense structural
diversity with characteristics of al1 areas of the periodic table. The atom adopts covalent-
type bonding cornmon to main group elcments, and can accommodate Lewis bases to
fom labile adduct complexes typical of transition metals, which may include
intramolecular interactions (e.g. amino-lesterthiolates). Bismuth is the heaviest non-
radioactive element, and its large atomic radius (1 S2A) allows for higher coordination
numbea (typically three to tm) and more variable goometries than those achieved by
transition metals. As a consequence, bismuth is capable of coordinathg larger
polydentate ligands (e.g. polyaminocarboxylatcs. larger cmwn ethers) and extensive
intermolecular bonding. Secondary interactions are mediateci through introduction of
sterically bulky Ligands (e.g. 2,4,6-tert-butylphenylthiolate), manipulation of the Lewis
acidity of the bismuth center (e.g. electron withdrawing pentafluorothiophenolates), and
utilization of bihinctional ligands (e.g. arninothiolates), suggesting potential utility in
supramolecular chemistry and development of novel materials. Further, structural
diversity results h m relativistic effects which inducc an unpredictably variable
stereochemical activity or inactivity of the B i 0 lone pair.
In addition to their fiindamentai intacsf smictural studits play a key role in
establishing and confïrming accurate formulae assignments. As part of the extensive
6 c haracterization of compounds prepared in this thesis, several other techniques have also
been utilized.
1.3 Characterization Techniques
A majority of the compounds in this thesis have been comprehensively
characterized in both the solid state (EA, mp, FT-innurd and FT-Raman spectroscopies,
X-ray crystallography) and in solution ('H and ''C NMR spearoscopy, and AeCI or ES1
mass spectrometry). In addition to X-ray crystallography, m a s spectmmetry and
particularly FT-Raman spectroscopy have proven to be usefil techniques for product
identification.
Bismuth compounds are typically therrndy unstable, that is they decompose
before melting, and are of low volatility. Thmfore, m a s spectrometry sampling
techniques which involve heating the sample into the gas phase under high vacuum, such
as electron impact ionization (ET) and chernical ionization (CI), an generally not ideal.
Atmosphenc pressure chernical ionization (APCI) (see Figure 1.3) and electrospray
ionization (ESI) provide the advantage of introducing the sample in solution and involve
minimal (APCI) or no (ESI) thermal heating. Moreover, due to the high sensitivity of the
mass spectrometer, minimai sarnple concentrations are required.
Bismuth compounds, particularly bismuth thiolates, are strong Raman scatterers
below -3SOcm", a spectral region that is not typically pmbed by inûared spectroscopy.
This provides an intense and distinctive hgerprint for idcntifyîng recovered reactants
and new products. In addition, the speed and minimal ample preparation quired in
Figure 1.3 APCI-mas spcetnmi of bis(hyboxycthaocthiolato)bismuth(IIT) nitrate 550 in
acetonitrile.
8 collecting spectra establishes FT-Raman as a valuable technique for studying these
cornpounds.
Complexes prepared and discussed h m i n have been chosm based on specific
cnteria To enhance readability of this manuscript, some brief comments regarding this
topic as well as some generai remarks concemùig forrnatting of this manuscript are
provided.
1.4 Scope of Tbesis and Geaeral Comments
Since, the majonty of medicinai chemistry of bismuth involves Bi(m), this work
concentrates on the trivalent chemistry. Although there have been examples of Bi(V)
complexes of tropolone derivatives prepared a s potential antimicrobial agents,'v6 these are
not discussed in this manuscript.
In keeping with a biomimetic theme, al1 manipulations have been pedormed
without exclusion of water. Because of their hydrolysis to bismuth oxides in aqueous
media and theu minimal role in medicina1 chemistry, organo-bismuth compounds
(compounds containhg bismuth-carbon bonds) are generally not discussed, except to
provide a comprehensive account of a specific subsection. Also excluded fiom
discussion are complexes which involve bismuth as a Lewis base (e.g. bismuth-transition
meta1 complexes).
Generally. drawings are intendcd to illustrate connectivity and the coordination
geometry of bismuth only [dashed lines (-) reprcsent long or intennolecular contacts].
Drawings of these compounds aimed ai describing bonding features, such as Lewis
structures, are not meaningful or are misleadhg for bismuth complexes, while they are
9 employed for the description of some ligands. Crystallographic figures are drawn with
50% probability themal ellipsoids.
Tables of characterization data are pmenteâ in discussions of established
compounds to demonstrate the favorabili ty of product formation (i.e. yield) and the
reliability of structural and formulae wignments. The following series of reaction
equations, which are refmed to within cach table, incorporate synthetic reactants
describeci by the original authors and are intended to illustrate the breadth of synthetic
approaches employed. Reaction balancing schemes and by-products are not meaningfiil.
Previously prepared compounds and substrucnires are numbered according to the
chapter in which they are discussed, followed by a two or three digit nurnber signifjmg
the order in which they appear in the chapter (e.g. 309 signifies Chapter 3, compound
nine). New compounds prepared as a focus of this thesis are numbered by chapter
followed by a sequential capital letter (e.g. signifies Chapter 7, second compound).
General structures and bonding situations are n u m b d sequentiaily throughout the
thesis and are labeled with upper case roman numerals (e-g. II).
1.5 Conclusions - Industry and the Scientific Method
Industrial influence on the sciences is evident in this work through the study of
rnodels of commercial phamaceuticals and deserves a brief comment. On the one hand,
the need for "practical" science generates new ideas and directions that would probably
not be considered otherwise. However, th- is o f h a societal rrpuirement for
immediate applications, and problems potentially vise when prematwe conclusions are
10 drawn. A compromise involves assessment of fiindamental attributes with practical
appiication in the foreseeable, but not necessarily immediate, fùture.
Bismuth containing prepatations and compounds have been used for over 200
years to treat a variety of medical disorders. As a prirnary industrial interest for bismuth
chemistry, the pharmaceutical utilization of bismuth compounds would lead one to
believe that the mechanism of action of these compounds is well understood and their
pharmaceutical usage validated. In fact, the serendipitous discovery and use of these
compounds has led to centuries of medical empirical support with minimal underiying
chernical basis for these observations, yet they are still widely used today.
This is not to insinuate that studies in this area have not been numerous. Despite
difficulties associated in working with bismuth compounds several observations have
been made, but with few comprehensive chernical studies or general conclusions.
Further, vague and false statements plague the literature and have bem utilized as a basis
for conclusions and hypotheses for fiuther studies. This "snowball effect" results in the
misconception of acquired knowledge, and, therefore, the importance of valid
conclusions based on accurate empirical observations without over-interpretation must be
stressed.
The logical approach to understanding more complex situations, such as
biological systems, is rational and involves simpler, more e a d y understood models. The
fundamental knowledge gained in the process does not only provide insight into the
irnmediate problem, but also any othcr complex systern that we hope to understand now
or in the future. This thesis embraces this appmach.
I l In the author's opinion, the attractivencu of the following work is in the
simplicity of the approach employed. Therefore, there is the potential for an increased
appeal to a wider scientific audience and a decline in the number of assumptions required.
Despite its simplicity, some very g e n d conclusions can be made regarding not only the
specific topics addressed in this thesis, but about the systematic approach employed.
12 Chapter 2. The Chemistry of Medieinal Bismuth Compounds: BydroxyJ
Alkoxycarbosylates and Inorganic Sdts
2.1 Introduction
The bio-utility of bismuth and its compounds has a 250 year history, which is
described in a number of key review articles,'-" but the appearance of bismuth
compounds in the British Phannaceutical code^,'^" the French Phar~nacopeia,'~ the
Gexman Pharmacopeiam and the new Czechoslovalcian ~harmacopeia," is more recent.
Some compounds have been appmved for human use under the F e d d Food, Dmg and
Cosmetic Acp for more than 30 y-. After extensive use in the treatments of syphilis,
as well as other bacterial infections, the heavy metal label effected a decline in usage with
the advent of antibiotics, and incidents of revmible bismuth encephalopathy in France
and Australia in the 1 960's and early 1970's. Nevertheless, bismuth compounds remain
important components of stomach remedies, such as ~epto-~ismol. (bismuth
subsalicylate, BSS) and ~ e - ~ o l @ (colloidal bismuth subcitrate, CBS), and derivatives of
CBS, such as ranitidine bismuth citrate (RBC), are cumntly under development.
This chapter provides an overview of the data available for prominent bismuth
compounds which have been discoverex& developed or designed to have biological (with
the exception of botanical) activity or medicina1 utility, while a more complete review of
the topic has been written.l> A number of compoimds have been sufficiently well
charactenzed to assign fomulae accurately, however, a wide variety of materials,
mixtures or preparations containing bismuth have been examined and docurnmted, many
of which have ill-defineci fonnulae or vague name designations. The chernical aspects of
13 cornpounds for which definitive fomulae or characterization data are available are
discussed and compared. Tables 2.1 and 2.2 are lists of compounds with Literature
references to each item of characterization data.
2.2 Inorganic Compounds
The earliest bismuth compounds to be used for medical purpose were inorganic
bismuth salts, typically the basic bismuth salts, such as bismuth subniüate (BSN), which
was known as early as the 17'" centuy as "magisterium bismuti"." and bismuth
subcarbonate (BSC). A listing including assigned formulae and references to
characterization data are given in Table 2.1. Some named compounds have a variety of
formulae (e.g. subcarbonate and subnitrate) arising h m the variable preparations,
procedures and subsequential characterisation. Their designation as 'sub' salts has likely
been justified on the basis of high oxygen content and the a s s imen t of Bi-O moieties.
Most formula designations are baseci on elemental analyses and maybe overïnterpreted,
for example, bismuth hydroxides are sometimes written as BiO(OH), but could be
bismuth oxide (Bi203) with variable water content.
Bismuth is mined as bismuth oxide (Bi,03, "bismite") as well as the sulfide
(Bi$,, "bismuthinite"), the former of which may be prepared nom other inorganic
bismuth salts (nitrate subnitrate, subchloride, sulfate) by reaction with a carbonate or
alkali hydro~ide=~~ or by thermal decornpositi~n,~*~' or by other methods including
heating bismuth metal with sodium nitrate and hydrolysis of bismuth a lko~ides .~
Bismuth oxide existr as a number of polymorphs. a-, &, y- and 6-bismuth sesquioxide
form at various temperatures and have been studied extensively by DTA9' and X-raf7
Table 2.1 Compound designations and assigned formulae for medicina1 inorganic
bismuth compounds.
compound designation fonnula re ferences
oxide (bismite) Bi203 37
h ydroxide 3842
carbonate 40.46.47
basic carbonate 48.49
subcarbonate 50
- basic bismuth nitrate 71-74
subnitrate 75
Table 2.1 Compound designations and assigned fomulae for medicinal inorganic
b i srnuth compounds (continued).
compound designation fornula references
chloride/ trichioride BiC1,201 82
oxychloridd subchionde BiOCl203 83
subiodide U
oxyiodide Bi01 8s
aluminate 86.87
Bi2(Al20J3m 1 0H20 88.89
and neutron powder di~~tion.~' The crystaI structure of the a-oxide3' shows parallel
layers of oxygen atoms with bismuth atoms located between them. The oxygen atoms
form a pattern of three and five sided polygons, with the corners king bridged by
bismuth atoms in a three dimensional lattice. There are two unique bismuth atoms, one
five- and one six-coordinate, in distorted octahedral envhnments, the latter of which has
a corner of rernoved. Each bismuth atom has three short Bi-O bonds [2.08-î.î9A] and
two or three longer Bi-O contacts [2.48-2.80A].
The chlonde (BiCl, 201)~ and nitrate [Bi(NO,),.SH,O 2021" sdts of bismuth are
typicall y prepared fkom the reaction of bismuth oxide with the conesponding strong
mineral acids, and have both been stnicturally charactaited. BiC1,201" is molecular in
the solid state, witb one unique eight coordinate bismuth ceater. Each bismuth atom has
three closely bound chlorine atoms pi-CI 2.468-2.5 18A] in a near pyramidal
16 anangement and five long chlorine contacts Bi-CI 3.2 16-3.450AJ The nitrate
pentahydrate 202,' on the other hand, is ionic in the solid state, consisting of Bi3+ cations,
NO3' anions and lattice water molecules. Here, bismuth is bound to one asymmetrically
[Bi-O 2.60(1) and 2.99(2)A] and two symmetrically p i - O 2.43(2)-2.66(1)A] chelated
nitrate ions, and four water moiecule oxygen atoms [Bi-O 2.32(1)-2.67(1)A], giving a ten
coordinate geometry.
In weakly acidic to basic conditions the inorganic salts are "hydrolysed" to the
corresponding oxide products, commonly refcrred to as "basic," "oxy-" or "sub-" salts,
which have a tendmcy toward the formation of the favorable BiO' bismuthyl subunit.
Such is demonstrated by the hydrolysis of bismuth chlonde in water to form bismuth
oxychloride:
2.1) i3iC13(s) + H20 BiOCl + 2 HCl
It has been argued that the solubility of BiOCl in acid species is not simply due to the
liberation of Bi" b m BiO' by the hydronium ion," but to the formation of the anionic
species ~iCl,? Supporting data include the greater solubility of BiOCl in hydrochloric
17 acid than in nitric acid, and the increase in solubility of BiCI, and BiONO, in nitric acid
with the addition of NaCI. Solution studies of the cornplexation of bismuth(m) with the
chloride ion encompass not only aqueous mediaM but also organic sol vent^.^^-^
Investigations into aqueous reactions of bismuth ~hlonde'" '~~ involve the effect of
temperature on hydr~lysis '~~ with formation of BiOCl203, BiOCI*2H20, and BiCI, *H,O
solid phases,'(" while the hydrolysis of bismuth subiodide has similarly been s t ~ d i e d . ~ ~ ~
The crystal struchue of BiOCl 203,1M the only sûucturally characterized hydrolysis
product of BiCl,, shows one unique eight cwrdinate bismuth center smunded by four
oxygen atoms and four chlorine atoms [Bi-O 2.3165(12) A] and pi-CI 3.059(8) A]. The
atoms create asymmetric decahedrons around the bismuth centers, which are linked in a
three dimensional array.
203
Unlike the hydrolysis of bismuth chionde, the lability of the nitrate ion allows for
a muc h greater range of hydrolysis products of bismuth nitrate,"s7ss107-' " with product
fomation (degree of hydrolysis) being sensitive to specific precipitation condition^."^'^'
The majority of these products have been identified by physical techniques, such as
chernical analysis, while species in solution have been detemllned by electrical
cond~ctivity."~
This sensitivity to &on conditions is dwonstrated by the fomation of:
[Bi,0,(OH),)(N0,),*3H20 204.~" (modified formula BiONOpO. 1Bi,[email protected]),
18
ob tained in the 1.2 to 2.4 pH range; slightly l a s basic [Bi,04(OH)4 ](N03),*H20
(modified formula [email protected]), isolated by crystaliizing Bi(NO,),*SH,O fiom
boiling O.OSM m O 3 or by heating crystals of ~i,O4(OH),I(NO,),a4H2o; and
[si60,(oH)4](No3),*4~ 204cZ4 (modified formula BiON03*H20), recovered as the
h t solid hydrolysis product below pH 1.2. The structures of al1 three compounds are
very similar and are composeà of [B~,O~(OH)J('@'"~ hexanuclear poiycation ciusters 204
204
with loosely coordinated bidentate nitrate anions and water molecules. The hexanuclear
units 204 show six bismuth atoms sitting at the corners of a slightly distorted octahedron
with the eight oxygen atoms capping the octahedron faces. The structure of
i60,(OH),] (N03),.3H,0 2 04 is composed of [Bi60,(OH),]" cages, which dimerize
through a Bi-O edge. The Bi-O bond distances fdl into three ranges, comsponding to
the Bi-O,,,, [î. 10(4)-2.23(3)A], Bi-Ob- [2.22(4)-2.52(3)A], and Bi-OWnI [~.ss(~)AJ
bonding situations. The stnicture of [Bi,04(OH),](N03)6.H,0 204bn-m contains a
monomenc hexacationic [Bi604(OH)4]* cluster with four oxide oxygen atoms and four
hydroxide oxygen atoms. A short Bi-O*, [2.62(3)A] and a short Bi-O,, [2.64(3)A]
contact gives two five-coordinate bismuth atoms. The structure of
[~~,O,(OH),I(NO,),@~H,O 204eU shows a simiiar arrangement.
19 Further evidence for the preferred formation of the bismuth-oxygm polycation is
its presence in the hydrolysis products of bismuth perchlorate in s~lution'"'~ and in the
so lid state in the hydrolysis product ~i604(OH)4](C104)p 7H20 204d.I"
Bismuth oxide itself may be hydrolyzed or hydrateci [e.g. Bi(OH), bismuth
hydroxide, BiO(OH)], and aqueous mixtures have been studied at various pH
v a i ~ e s . ~ ~ ' ~ ~ ' ~ ~
Bismuth carbonate may be formed h m the reaction of Bi203 with excess CO,, or
the reaction of Bi(NO,),-SH,O with excess Na&03 or K2C03."-"JU5 As with bismuth
subnitrate, the composition of bismuth subcarbonate is sensitive to reaction conditions.
This accounts for references to "light" and "heavy" bismuth subcarbonate and subnitrate
in the phamaceutical and medical literat~re,'~' which exhibit variable therapeutic action
depending on basicity and degree of subdi~ision.'~'
"Bismuth aluminate" is a variable composition of Bi203, N,03 and H,O and
possibly CO,. It is employed maidy as an antacid, combining the antacid properties of
the basic bismuth and aluminurn oxides.
Of the inorganic salts employed in medicine, only bismuth chloride, oxychloride,
and nitrate pentahydrate have definite compositions. The variability in the subnitrate,
subcarbonate, hydroxide and aluminate results h m the sensitivity of product formation
to reaction conditions. This variability in composition may account for variability in the
2.3 Carboxylates and Derivatives
2.3.1 Hydro~carboxylc Acid Complexes
Bismuth complexes of hydroxycarboxylic (aliphatic hydroxy acid) acids,
including galiic (Ha, tartaric (FI&), lactic 0, malic (Hgai), and citric ( H m
acids, have been used in a wide range of medicinaî capacities since the tum of the
century. An ovemiew of the characterization data that have been obtained for isolated
bismuth polyhydmxycarboxylates is pnsenied in Table 2.2.
As with bismuth subnitrate, the lability of the bismuth-carboxylate interaction
allows for variable compositions of these compounds, which are very sensitive to reaction
condition^.'^^*'^'^ Moreover, the fonnulae arc somethes speculatively wigned on the
basis of preliminary identification.lY There have becn two crystallographically
2 1 Table 2.2 Characterization &ta for isolated bismuth hydroxy-/alkoxycarboxylates.
Compound designation
Formula Characterization Data
basic bismuth EA'33 gallate
gallate E A ~ ~
Na Bi Gallate prep, EAt3'
Na Bi Digallate prep, EA'~'
Na Bi Me Gallate prep, EAl3'
oxyiodogallate C,H(OH),(CH,)COOBi(OH)I prep,136 mp137.138
"Airo1"
iodogallate DTA'~'
tartrate PreP, 139 ~ ~ , 1 * 1 " IR143
acid
bismuthotartrates lRt~s
sodium ûibismuth COO(Na)CHO(BiO)CHû@iO)COO- pnp" tartrate
sodium bismuth PreP, 147 ~ ~ , 1 4 8 ~ ~ ~ 1 3 0
tartrate
d- and meso- BiO(H&@nH,O, prep, IR'"
d-Bi(H&g)(Hm .3H20, dl-MBiO(H& and M B i w
B i ( H a ( H a . 3 H 2 0 prep, EA, XRHO
MBi(Hw (M = K, Na, Li, NH,, Hpy) prep, IR"'
KBiO(H&), K B i W p q , IR152
Bi2H2(&),, NaBi2O2HW prep, EAlS3
Table 2.2 Characterization data for isolated bismuth hydroxy-Ialkoxycarboxylates
(continued).
Compound Formula Characterization Data designation
NaBiO(Ha, Na(BiO),m P ~ V ' ~
Bi2(Hw3*2(H&) prep155
Bi Na acid tartratc prepI6
sodium potassium EA"~ bismuth tartrate
prep, XR1"
bismuthate(III) hydrate
malate Bi(pab*H20 prep, EA, XR'"
citrate prep, EA, 14' DTA' 'O
Bi(Hç-) P ~ V "
Bi(H&) aH20 prep, ïR, DTAI6'
Bi3(Hcith(OK)3 prep, EA'"
"pentabismoi" 16NH,OH. 1 lBi(H&).Bi(OH), P W ' ~ ' "
*6H,O
bismuthocitric acid ~ r r ~ ' "
sodium bismuth P~V" citrate
23 Table 2.2 Characterization data for isolated bismuth hydmxy-/aikoxycarboxylates
(continued).
Compound Formula Characterization Data designation
dibismuthyl sol'* monosodium citrate
characterized bismuth tartrate compounds, which arc isostnictural and involve two five-
membered bidentate chelate ligands. In the ammonium salt, NH4[Bi(H,tar)Z(H,0)] .H,O
205,"' four bidentate doubly deprotonated tartaric acid ligands surround each bismuth
center. The two crystallographically unique ligands an bound to the bismuth center via a
carboxylate (O1) and an a-alkoxide (e) oxygen atom Pi-Odx,, 2.372(7) and
2.438(6); Bi-Odw* 2.462(6) and 2.460(6)A] fomiing five-membered rings. One of these
ligands bridges a second bismuth center in a similar manner via its remaining carboxylate
(O6) and the a-hydrox y (O4)groups Pi-O,*, 2.608(6), Bi-O-YIK 2.622(6)A]. This
carboxylate group asyrnmetrically chelates a third bismuth center in an 0,O' (os, 06)
manner ~i-Oo,,~-,,,,x,,k, 2.476(6) and 2.738(6)A] forrning a four-membered -BiOCO-
ring. The oxygen atom of a water molecule completes the coordination sphere [Bi-O,,
24 2.400(6)& for a total coordination number of nine around bismuth and a ûigonal
prismatic geomehy. The resulting structure is a complex one-dimensional coordination
po lymer with extensive hydrogen bonding. The complex B i(H&&(H&Q.3H20 206Is0
contains a singly deprotonated (Hm- tartrate Ligand, but retains an analogous structure
to the ammonium salt [Bi-O-* 2.381(10)-2.615(11); Bi-Omy 2.467(9)-2.588(10);
Bi-Oo,,.-x, 2.482(10) and 2.754(11); Bi-O, 2.409(9)&
There have been several solution studies of bismuth tartrate compounds and
systems 148.173-1 75 emplo ying several spectroscopie and physical t ethniques including
vi~ua1, '~~ spectrograp hic1" and solubility methods,"' optical rotation @-tartrate), ' " ' H
NW 17' polarirnetxy, 174.177.179 p~tentiometry,'~'" p o l a r ~ g r a p h y , ~ ~ . ' ~ ' ~ ~ e lect r~rnetry '~~~~~'
and o~cillography.'~~ These approaches have been employed to detennine the
corn position^^^^^'^ and stability constant^'^^^^^"^ of complexes at a variety of pH
valUeS 180.1 8 1, '861 88 and at various tartrate con~entrations.'~~~" mer investigations involve
extraction of bismuth tartrate complexes nom solution using diisoamyl amineIag and
hydrolysis studies with the isolation of NaBiO(Hu and Na(BiO),(tar) sodium bismuth
"sub"tartrate cornplcxes. lw " Few bismuth compounds of lactic acid (Ha have been
reponed.lU.IS8.1J9.162.163.191.192 Bi(Hlac), 207,'~' the ody structurally characterized example,
shows three chelating lactate ligands, dl of which are singly deprotonated at the
carboxylate fûnctionality and fonn five-membered -BiOCCO-rings. Two of the ligands
are tightly bound [Bi-O,, 2.205(7) and 2.364(8); Bi-Oh*y 2.474(8) and 2.457(9)A],
while one is weakly bound [Bi-OWy, 2.628(9)& Bi-OhWy 2.800(1)A]. The
carboxylate group of the weakly bound ligand coordinates a second bismuth center
25 asymmeeicaily in an O,Ofmanner [Bi-O 2.328(9) and 3.104(9)& forming a four-
membered -Bioco- ring. The exocyclic carboxylate oxygen of a tightly bound ligand
coordinates a third bismuth center [Bi-O 2.580( 1 )A], giving each bismuth atom a total
coordination number of nine and an overall complex three-dimensional network structure.
A mixed lactate-tattrate complex dilactatobismuthotariaric acid C,J-i,,O,,Bi has also been
prepared nom the reaction of lactic acid with Bi nitrato tartrate,'" while no solution
studies of bismuth-lactate systems have been reporteci.
As with lactic acid, few bismuth complexes of malic acid have been
prepared. 162.191 The single stmcturaily characterizcd exarnple Bi(mai)aH,O 2 0 8 ' ~ shows
bismuth chelated by four triply deprotonated malate ligands in various modes pi-O3
2.244(6) and Bi-O' 2.407(8)A; Bi-O' 2.255(6) and Bi-0' 2.571(9)A; Bi-O' 2.959(9) and
Bi-o2 2.553(8)A; Bi-O' 2.351(9) and ~ i - O s 3.233(9)A] fomiing a five-membered, a six-
membered, and two four-membered rings. The oxygen atom of the lattice water rnolecule
pi-O,, 2.80(1)A] completes the coordination sphere for a total coordination number of
seven. The bonding of each ligand to four bismuth atoms again rrsults in a highly
coordinated polymeric network.
Few solution studies of bismuth-maiic acid systems have been performed and al1
involve physical methods, including ele~trometr~,'" polarirne~y,'~~ p~larography,"~
oscillography1" and a bismuth ion-selective electrode.'" Stability constants"' have been
detexmined at various pH and malic acid concentrations. lg3
2.3.2 Poïyaminocarboxylates and Tliioiatocarboxylnres
In addition to hydroxycarboxylic acid complexes, bismuth complexes of the
polyaminocarboxylic acids nitrilotriacetic acid (Hm, also commonly referred to as
triglycollamate, and ethylenediaminetetraacetic acid (Hm have also been employed in
medicine" and pharmacy and studieû phamia~ologically.'~~ Similariy, a number of
bismuth complexes of the thiolcarboxylic acid ligand H m have been assessed for
pharmacological'96 and antimicrobial activity. Synthetic and structural data for isolated
bismuth Bi-- and Bi-sdta complexes is presented in Chapter 4.2.
HOOC, /-\ +00H
HOOC N N OOH HOOCJ ~ O O H
27 There have been several studies of Bi-- complexes in sol~tion,'~' at various pH
and employing both ~pectroscopic '~"~~ and physical"3.'9"w0'50
techniques. A number of physical constants have been determined for these systems
including f~nnation,'~' stability,'"3*'9g2003033205 protonati~n,~~~ hydrolysi~;~~ and rate
constant^,'^' as well as dissociation potentials2& thamodynamic f û n c t i o n ~ ~ ~ ~ and
mechanism of complex formation? The interaction of and edta with BiCl2- has also
been studied. For the bismuth-& system, both s p e c t r o s c ~ p i c ~ ~ ~ ~ ~ ~ ~ and
physical 183. I8SMl20C2O7,2W,.2"PI techniques have been employed to detennine complex
composit ions~ dissociation potential~?~ molar ab~orbances,2"~ and
stability, I832ûbZ05207tl I.ZIV~Z-224 protonation constants,'OS as well as hydrolysis constants20s
and k i n e t i ~ s . " ' ~
Isolated bismuth complexes of thioglycolic acid include bismuth dithioglycolic
acid,=' ~i,(tga)~ca,,~~ ~ i ~ ( t i t g â ) , = ' Na Bi thi~glycolate,'~
ethylbisrn~thothiogiycolate,~% and Bi thioglycolate-triamide,'% while Bi-tgê solution
systems have been studied by spectroscopie techniques ~ n l y . ~ '
2.4 'ColIoidal Bismuth Subcitrate' (CBS), 'Bismuth Subsalicylate' (BSS) and
'Ranitidiae Bismuth Citrate' (RBC)
Citrate salts of bismuth represent the most extensively studied series of bismuth
compounds by virtue of the widespread medicina1 use. Bismuth citrate is essentially
insoluble in water, but a dramatic increase in solubility with increasïng pH has been
exploited as a bio-ready source of soluble bismuth, a material referreâ to as colloidal
bismuth subcitrate (CBS). Formulation of these solutions is complicatcd by the
28 variability of the bisrnuth:anion stoichiometry, the presence of potassium a d o r
ammonium cations, the susceptibility of bismuth to oxygenation to Bi=O and the
incorporation of water in isolated solids. Consequently, a variety of formulae are
classified in the literame as CBS. [ J ' v ' J 4 . ' 6 2 - ~ ~ . l 6 6 . 1 6 7 . I ~ U o ~ Solutions have been examined
by a variety of approaches, including visual studie~"~ and physical 1 8 3 - I B S . I W . I ~ ~ . Z ~ ~ , Z ~
techniques, to determine corn position^'^^^ and stability constant^'^' of bismuth citrate
solution complexes. at various p~"'*'" and citrate concentration^.'"'^^ ' H and I3C NMR
spectroscopy indicate rapid exchange of citrate moieties at low concentration and
the existence of oligomeric or polymeric units at higher concentrations.
Solids isolated fiom various, often ill-defined combinations of bismuth citrate,
ch i c acid, potassium hydroxide or ammonium hydroxide have been assigned formulae
on the basis of elemental anaiysis data or by determination of water and ammonia
Additional speculation is made for their presentation as modified fomulae
(& = C,H,07'-; H& = [C02CH2C(OH)(C0&H2COJ3-), however, assignments for such
complex systems are of low significance in the absence of complementary data other than
thermal analy~is,~' infiard spectroscopp7 or NMR spectroscopy."' In this context, the
Merck index lists the chernical fonnula of CBS as K,(NH,),i)i,O,(OH),(Ca,O,), in the
1 lth e d i t i ~ n , ~ ~ but in the most recent edition provides a less precise name 6'trip~tassium
dicztrato b i smu~hate"~~.
More defmitive formulae have been detemiined by X-ray crystdlography and are
listed for structural cornparison in Table 2.3. The conditions for isolation of these
crystalline materials fkom solutions similar to those denned above are provided in some
cases, but are sometimes incomplete and often involve time periods of months. Isolation
29 of the sodium salt 213 was somewhat unusual in that it was unexpectedly obtained fiom
reaction mixture of ranitidine bismuth citrate, glutathione, D20 and NaOD?'
The structures in Table 2.3 are al1 closely related and are generally composed of a
citrate anion (çif) intimately bound to a bismuth center, an appropriate number of
potassium or ammonium cations (to balance the charge) and solvated or coordinated
water molecules. Thme of the structures 214-16 contain an additional citrate trianion
(Hçir = C6H,0T) and one stnicture 216 is constnicted around a hexanuclear bismuth
oxygen cluster @&O,), similar to that found in bismuth subnitrate (204). The
stoichiometries of the components are variable, including the bismuth citrate relationship,
but most involve a well defined chelate interaction with the tridentate citrate bismuth
complex. The potassium and ammonium cations are essentially interchangeable, and the
ammonium salt 21 1 is isostructural with compound 212. The variety of reported
structures is somewhat misleadhg when one recognizes that of the eight structures listed
in Table 2.3 (nine structural types have been previously incomctly propo~ed'~), only
compounds 214-16 c m be considereà unique. Structures 209-13 are constructed from the
simple monoanionic complex. composed of Bi3* with a tridentate citrate tetra-anionic
ligand. This unit is also evident in 214-16, but these structures involve additional
Table 2.3 X-ray crystallographic data for soli& described as colloidal bismuth
subcitrate.
Formula Bi:& Coord Space Ce11 ratio # at Bi Gmup param., a, b, c, P
K(Bi&(H,O), 2OP4' 1:l 9 P2,h 10.924, 15.280, 14.967, 1 05.48
%.5(NH4)0.5(sim@20)3 3 1 p 1:l 9 P2'/n 10.923, 15.424, 15.037, 105.67
(MII)(B~&)(H~O)~ 21 1''' 1:l 8 C2/c 16.805, 12.544, 10.401,91.27
k.5(NH,)a5(siW(H20)2 212- 1:l 8 C2k 16.860, 12.395, 1O.328,9 1.79
N~(B~&,(H~o), 2 1 3 ~ 1:l 8 C2/c 15.723, 13.899, 10.423,94.39
L.,S(NH~)~S(~~UOZ(H~(HZO)I~ 214U3 2 3 9 P- 1 1 1.801, 12.973, 15.856,98.15, 108.39, lOO.9l
(NH,),@ici~)(Hcit)(H,O), 2 W 3 1:2 8 P2,k 8.998, 9.492, 27.021,99.42
(NH,)6(Si604)&4(HZO)I 2 16 235343 3:2 R-3 17.807, 17.807, [initially assigned 3 1.596 (NH4)6(si604oH)&(H,0)5Ha
chemically different units. This unit together with one or two cations and three or six
water molecules, defines the asymmetric unit of compounds 209-13, but adopts a well
defined dimeric arrangement imposed by chelate coordination of the pendant carboxylate
moiety to a neighbouring bismuth centcr. Différences in the macrostructures of
compounds 209 and 210 (P2,/n) and 21 1-13 (CUc) result h m distinctions in the
interactions between these dimers, which is likely only a fiinction of the degree of
hydration, i.e. the number of water molecules coordinated to bismuth. Compounds 214-
31 16 aiso involve the tridentate coordinatcd citrate tetraanion 0. However, the presence
of an additional citrate trianion (H& = [C02CH2C(OH)COtCH,COJ*), and an additional
citrate tetraanion for compound 214, cornpikates and opens the structures, enabling the
incorporation of additional water. Nevertheless, the familiar pendant carboxylate bound
dimer is evident in 214 and 215. Although compound 216 does not display the distinct
dimer unit, the tridentate chelation of one of the N o unique bismuth centers is clear.
The ubiquitous tridentate citrate chelation of bismuth, which has also been
observed for aluminum citrate complexes,"' implies a special stabili ty for the
b i scarboxylate/alkoxide interaction enforcing a pendant carboxylate. The coincident
coordination of this third carboxylate is precluded by the required tetrahedral geometry of
the central carbon center of the citrate anion. The consequential five- and six-membered
chelate heterocycles are favoured over two seven-mernbered heterocycles imposed by
coordination of three carboxylate oxygen atoms. More importantly, the alkoxide has a
substantially higher basicity than the carboxylate. In the carboxylate chemistry of
bismuth, the citrate salts are uniquely water soluble at high pH with avoidance of
hydrolysis, which typically gives Bi0 for other salts. The tridentate chelate involving the
alkoxide dominates this behaviour relative to other polycarboxylates and relative to
bismuth citrate [Bi@?&)] at neutral or low pH, which is deprotonated at high pH.
The very low solubility of bismuth subsalicylate (BSS) has hindered
charactensati~n,'~*'~~ while the more reccntly developed ranitidine bismuth citrate (RBC)
217, a new therapy for peptic ulcer diswe, is highly water-soluble. RBC is obtained
fiom the reaction of ranitidine hydrochloride [N,Naimethyl-5-(3-nitromethylene-7-thia-
2,4-diazaocty l) hican-2-methanamine] and bismuth citrate. Characterization has included
32 elemental analysis, 'H and "C NMR and IR spectmscopy, polarography and X-ray
powder di fn-action, however, definitive structural assignmmt has been complicated by
extensive hydrogen bonding. The proposed structure is speculated to involve the
formation of a five mernbered ring by chelation of the bismuth center by NMe, and
salicylic acid (Hîsal) rani tidine
2.5 Models and Alternatives for Bioactivc Bismuth Compounds
The apparent chernical complexity of the commercial bismuth containing
phannaceuticd agents, which is imposed by the lability of the ligands has prompted the
development of simpler mode1 compounds and the search for alternatives to the
established systems. Therapeutic or anti-bacteriai activity has been speculated upon or
suggested for many bismuth compounds, and some have been assessed in vivo and/or in
vitro. Table 2.4 lists examples of compounds for which a medicina1 effect has been
suggested or evaluated, together with the preparative method. Most compounds of this
type are superficially chancterizd and the molecular structures or even the fonnulae
have not been defked, with some cases illustrating varying composition depending on
speci fic reaction condition.24uw
33 Systematic and comprehensive synthetic studies have recently been coupled with
bioactivity snidies to confirm the bio-significance of bismuth and reveal important trends
in activity. Extensive series of bismuth (Xi) and bismuth (V) tropdones and bismuth
(III) thiosemicarbazones and dithiocarbazonic acid methylester derivatives have been
assessed for their anti-HelicobacterpyIori activity illustrating a substantialiy lower
minimum inhibitory concentration for the f~rmer .~
tropolone thiosemicarbazone
As a heavy metallic elemmt, bismuth has a prominent thiophilicity responsible
for the facile fornation of sulfido and thiolato complexes, and a consequential
thermodynamic and kinetic stability, which has enabled synthesis and isolation of the
most extensive array of denvatives. Numemus examples have been assessed for their
bioactivity, but more irnportantly systematic series of compounds have been prepared and
evaluated. Antimicrobial bioactivity assessrnent of three systematic senes of
comprehensively characterised thiobismuth compounds, 2 17,2 182 and 21 9) (syntheses
and characterization of these compounds are dimwed fiuther in Chapter 5.3), against
CZostridiurn dtJTcife, Helicobacfer py lori, Escherichia col& Pseudomonas aemginosa and
Proteus mirabilis reveals significaat differcnces in activity across each series, suggesting
a structure/activity relationship for the bismuth environment.' In addition, a rat mode1 of
gasûic ulceration has revealed distinct differences in the ulcs healing efficacy of the
Table 2.4 Examples of other bioactive bismuth compounds.
Compound formuia Chernical (BioJ Suggested or Ref designation Med.) Dam evaluatcd
medicinal efkct (Mode of AAmin.)
phenylbismuthbis PhBi(Cfi4N0S), p r q ~ (in vino - dctcrgents, soaps, (2-pyridinethiol grun positive, shampoos 2s 1
1 - oxidc) gram negative)
organobis(thio- C&@@C&C~-P)D prep, Jpecttoscopy bactericide 252
phenylato) CH3Bi(SC6H4NH2-~)~ bismu th(m)
m-1 r m ~ 3 i ( s c d r ~ ~ ~ r n ~ - ~ ~ r , [CH~B~(SC~H~NH~CH~-PW W 3 I 2
3-phenylthio- and Bi salts of Pfcp ulccn s 3
phcnylsulfonyl- RC,H,S(O),CH=CHCO,H (cytoprotec tive acrylic acid (R = H; halo, C,, alkyl or alkoxy, aad gascric acid bismuth salt NO,; n = 0.2) secretion-
inbiiitory)
p-chlorophenoxy- mono- and bis- PreP depressan t for 2s
isobutyric acid ~CI(C~,)OC(MC)~CO,H salts blood cholcstcrol bismuth salt
bismuth Bi(SC&i4CONH3, P m * sol (ointments, talc) 35
O-mercapto- (fiiagicidal, benzamide bactcricidal
activity)
dipropylacetic acid Bi[(C,H,),CHCOd, P m , mP, sol throat infections bismuth salt (rectal suppository
witb cocoa butter)
p-amino- and p- [Bi(C,HSIJO,),) 1, Prtp nibcrculostatic m berizamidosalicylic [Bi(C,,H,a04)J12 acid bismuth salts
bismuth O-AcOC&CO~iO pmp (stable in intestinal (oral. 2 s
subcompounds stomach - no data) rectal)
bismuth C4HJN40,aBi(OH)2 Pr- external and 3 9
allantoinate intemal ulccrs, wounds, etc.
basic bismuth C&(OH)(OCH,)CûûBiO prep, sol syphilis a50
guaiacol- (ointment, carboxylatc subcutancous)
bismuth hydrox y- Bi(OH),ûC&N PrcP, sol (antiseptic on 26 I
quinolinate wounds)
double iodide of w t i n e e 2 ~ ~ a 1 P m , (gehtin capsules) as emctine and bismuth
ethylene = (CHJJ derivatives of compounds 217 and 218.2a
I Bi \
S \
R R Bi-S
\
S, ,S R 's'
2.6 Interactions with Biomolecula and Pbumaceutical Agents
One proposed mode of action of mti-ulcn bismuth compounds is the ability of
bismuth to bind to proteins of exposed tissue and provide a protective coating over the
~lcer.~' It is crucial, therefore, to have an understanding of the bismuth bonding ability
of amino aciàs, proteins, and other biomolecules, which may also provide a basis for
conclusions of phamacological and pharmacoicinetic snidies. Further, bismuth
complexes of amino acid derivatives, such as D-peni~illamine~~ and other
dialkyl~~steines ,~~ have been suggested for medicina1 use, while polypeptide complexes,
such as those of glutathione, have been suggested for tteatment of syphilis and other
disea~es."~ Investigations of systems and isolated wmpounds incorporating bismuth and
amino acids or other biomolecules are described below.
2.6.1 Amino Acids
The bismuth methionine complex ~ i - 1 2 ~ was prepared in non-aqueous
media and chanicterized mainly by infked spectroscopy. The reaction of a slight excess
of cysteine ( H a , which contains a thiol fiinctionality, with bismuth subcarbonate in
3 6
aqueous media gave Bi(ÇrsH)pH20, in which the ligand retains one labile proton.*"
This compound was also characterized mainly by idhred spectroscopy. A bismuth
R = H, glycine
O I O H
= (CH&NH2, lysine = CH20H, serine = CH2SH, cysteine
R m 2 = CH2(CH3)tSH, penicillamine
= CH2CH2SCH3, methionine
cornplex of D-(-)-pdcillamine [ B i ~ C l ] , a cysteine dimethyl derivative, has
been structurally characterized and is discussed fhther in Chapter 5.3?
Solution studies of bismuth amino acid complexes include amperometry of
bismuth-glycine complexe^,^" spectrometry of cysteine complexes~" pH-metric
investigations of L-lysine complexe$" and polarognphy of serine complexes2".
2.6.2 Peptides and Proteins
The complexation between RBC and the tripeptide glutathione WH) (y-L-Glu-L-
Cys-Gly) has been studied in both aqueous media and in red blwd cells via 'H NMR
s p e c t r o s c ~ p ~ ~ " ~ ~ ~ and sulfur has been found to be the sbongest binding site for bismuth.
Stability constants have been detexmined for the Bi(&), species, and binding was found
to be cornpetitive between @H and ieQfê and is pH dependent.
glutathione (&H)
37 The binding of the Bi3' cation to hurnan senun transferrin @TF), an iron transport
glycoprotein, has been examined by W-vis and NMR spectroscopies,2n27' while the
effect of the concentration of bismuth on plasma protein and red blood ce11 binding, as
well as bismuth binding to human senun albumin, bovine serum albumin and hurnan
S e m , have also been studied?) The interaction of CBS with erythrocytes and
erythrocyte lysate has been investigated using 'H spin echo NMR2.0
The binding of tripotassium dicitrato bismuthate to the bile acids has been
investigated in vitro using 'H labeled acids and measuring radioactivity at high and low
PH."' Bismuth was found to bind each acid to varying degrees and only at low pH (2.0),
suggesting a mode of action in ulcer healing. Pepto-Bismol, as well as its individual
components bismuth subsalicylate and montmorillonite, have been found to sequester bile
acids fiom aqueous solutions in vitro."' Other studies examine the effect of pH on the
formation of bismuth protein complexes2u and bismuth-gelatin c o r n p o ~ n d s ~ ~ the
interaction of bismuth compounds with alkaline protein solutions under the biuretic
reaction condition^.'^^ and the behavior of elemental bismuth with various proteins under
anaerobic conditions. 286.287 Bismuth compounds have also been found to retard the action
of enzyrne~.~"
Bismuth salts are widely used in the catalysis of organic reactions, such as the
hydrolysis of nbonucleic a d s to dinuclcoside phosphates28sm and the production of
prostaglandins.293
Bismuth(m) has been found to form a saturateci 7:l complex with rat liver
metallothionein (MT), with sirnilar rr~ults for other metal ions, suggeshg linte binding
specificity for bism~th. '~ There has been a debatc over whether the proteins binding
38 bismuth are related to MT, so aitemative terms such as 'hietailothionein-like proteins
(MTP)" and " rend metal binding proteins (RMBP)" have been ~sed.*~' Isolation,
separation and amino acid analysis of these proteins showed that they were different fiom
cadmium induced rat MT.295 These bismuth induced RMBPs in rats have been divided
into two major components which have been studied spectroscopically? The hepatic
protein spectra show preâominantly zinc thiolate transitions, while the m a l protein
transitions c m be accounted for by botb bismuth and copper thiolate binding sites.
2.6.3 Interaction of Bismuth Compoundr wirh Other Dugs and Food
Components
Many studies have been dedicated to detennining the effect of medicinal bismuth
cornpounds on the activity of other medicinal components, or vice versa, in vitro, and in
vivo to evaluate àrug bioavailabilities. Many dmgs have been found to adsorb on
inorganic bismuth salts employed as an tac id^,"^'^*^ while adsorption does not occur
between al1 bismuth sdt-dmg combina t i~ns .~ Other in vitro shidies involve the
adsorption of dia~epaxn,~*' anticoagulantsU# and preservativesw7 on both inorganic and
organic bismuth salts.
Antacid bismuth salts rnay also have an effect on the and
excretion3" of other dmgs in the body when takm concumntly. Bismuth subcarbonate
has been fond to have a variable effect on the antimicmbial activity of various
antibiotics in vitro. 314315 Conversely, biologicdly active molecules may have an effect on
the therapeutic action of bismuth ~al t s ."~ The bioactivity of bismuth compounds
(thiolopnves) is inactivated by molecules containhg thiol groups, such as cysteine,
39 sodium thioglycolate, and sodium thiosuWate, while it is una.Eécted by sulfide and
thioether containing molecules, such as cystine and methionine."' While it has been
reported that penicillin is decomposeâ by bismuth ions in the pmence of water,"' there
were synergistic effécts observed between bismuth compounds and penicillin, which has
no activi ty alone, against T~panosontn equiperdum infectecl
The formation of soluble chelates of bismuth has also been studied in various
drugs and food~.~*' Atomic absorption studies show an enhanceci solubi lity of insoluble
bismuth salts in the presence of certain dmgs and food components including
polyalcohols, hydroxycarboxylic acids, ascorbic acid, aspirin, tetracyclines, vinegars,
h i t and citrus juices3" The effect of the complexation of a variety of antibiotics on the
migration of Bi3+ has been determineci by papa chromatography and
electro~hromatography.~~ Other bismuth-biomolecule solution studies involve
chlorophyll, phe~phytin,'~ D-mannit01~~~ and ascorbic a ~ i d : ~ . " ~ while complexes of
uracil and thiouracil,"' mucate, saccharate and other polyhydr~xcarboxylates~~~ have been
isolated.
2.6.4 Antidotes
Many ligands have ais0 been used as antedotes for bismuth poisoning. Chelating
ligands such as British anti-Lewisite ( H m (2,3-dimercaptopropanol),
ethylenediarninetetraacetic acid (H,edta), paminobcnzoic acidJg and cystine3" offer
some degree of protection against common medicinal bismuth compounds. Mucin
solutions have been suggested as a possible antidote aAcr ingestion of toxic metal
compounds as mucin solutions precipitate the metals h m suspensions of BiOHCO, or
British anti-lewisite (H3m other metals at low pH.''' A series of dithiol ethm have bcen synthesized as chelators
for heavy rnetals, fonning complexes of lower to~ic i ty .~ '~ British anti-lewisite has been
found to chelate bismuth strongly mough to react with bismuth ~ulfide,"~ while studies
of bismuth-u compounds involve stability rneasurements in cornparison to other dithiol
ligands3" and employ polarography."' FuRher, Bi-~dta"~ and Bi-bis! complexes337 have
also been assessed for antimicrobial activity in vitro and in
2.7 Conclusioas
The vast array of medicinal or anti-microbial uses for bismuth compounds
indicates a diverse biorelevance for the element, which is likely valid, but has not yet
been unequivocally demonstrated. A wide selection of compounds and complexes of
bismuth have been investigated for potential bioactivity without justification other than
bismuth content. Some therapeutic utility is best described as 'suggested', and most
experimental studies are impeded by the chernical complexity of the bismuth compound
or the superficial chernical knowledge base that is currently available for bismuth. Most
importantly, few definitive identifications of bio-bismuth interactions have been reported.
Nevertheless, the unquestionable antirnicrobial activity of some bismuth compounds at
low concentrations, the relatively low elemental human ce11 cytotoxicity, and the il1
defined gastric cytoprotective properties of certain bismuth salts highlights the chemistry
41 of bismuth as an important focus for the development or discovery of new phannaceuticai
agents. The efficiency of such developments will depend on the systematic assessrnent of
bismuth chemistry as a foundation for understanding biochemical interactions.
42 Chapter 3. Toward the GeneraI Syathesis of Bismuth Dicarboxylates and the
Structural Cbaracterization of Bismuth Oxalate
3.1 Introduction
As discussed in Chapter 2, emphasis in medichal bismuth chemistry has been
placed on bismuth salts of carboxylic acids and hydroxycarboxylic acids, of which
colIoidal bismuth subcitrate (CBS) and bismuth subsalicylate (BSS) are the most obvious
examples. However, the characterization of bismuth carboxylates is hindered by their
hydrolytic in~tability,~' the lability of the ligands in solution and the consequential
sensitivity of the conditions for isolation of solids. Also, the ability of the carboxylate
functional group to achieve extensive intemolecular contacts is responsible for complex
structures in the solid state and likely in solution. The medicinal importance of bismuth
carboxylates has prompted extensive studies of complexes involving simpler ligands
including lactate161, tartrate"*"' and malate'w, al1 of which have been characterized by X-
ray crystallography. Although the solid state structures of the simplest bismuth
monocarboxylates (i.e. formate, acetate) have been detennined, bismuth oxalate (the
simplest dicarboxylate) has only been superficiaily characterized as a guanidinium sait?'
This chapter out lines approaches to minimiMg hydrol ysis and enabling isolation
of bismuth complexes of simple carboxylate ligands. These developments have led to the
isolation of the parent oxalate salt, which has been structurally characterized as bismuth
oxalate octahydrate 36. Section 3.2 provides an overvicw of the data available for mono-
and dicarboxylate complexes of bismuth.
43 3.2 Syntbesis and Structure of Bismuth Carborylatcs
Characterization data for both carboxylate and dicarboxylate compounds of bismuth
are contained in Table 3.1, followed by reaction equaîions for synthetic procedures. Yields
are typically not reported and fonnuiae assignments are based on single aystal X-ray
difkxtion studies. Most compounds sublime rather than meit, therefore rneasurement of
sublimation point (sp) is indicated. Therc are examples of formally molecular and anionic
species and Lewis base adducts (e.g. 301,313 and 317, ncspectively), as well as an example
of a mixed alkoxiddcarboxylate complex (318). Structural details are iilustrated below.
Bismuth carboxylates are typicaiiy prepared by reaction of a basic inorganic
bismuth compound with concentmted carboxylic acid under reflux conditions, while the
anhydride is often introduced to remove by-product water. These compounds may also be
prepared by similar reactions with BiPh,, while partial metatheses give organo bismuth
carboxylates. Ligand exchange reactions with bismuth acetate (reaction 3.2), in particular,
have been extensively utilized to prepare a series of bismuth tris(monocarùoxy1ate) species
301 and 3 0 3 - 3 1 0 . ~ ' " ~ ~ The synthesis of w i (CF ,Cûû) , 1 312= (reaction 3.6) is unique
in that it involves the reduction of pentavaient bismuth. The two thiourea adducts of
bismuth acetate ~i,(CH3C00),&&(HZ0)] 316 and (Bi(CH3Cûû),@g)3] 317 are prepared
fiom similar reactants under different isolation conditions. The favorable
hydrolysis of bismuth carboxylates d o w s for the preparation of the acetate oxide or
"subWacetate [BiO(CH3C00)] 319 by dilution of a solution of Bi20, in acetic acid and
distillation of the excess acid? Other "sub" carboxylates, including [BiO(RCOO)] (R =
44 Table 3.1 Analytical dah for carboxylatc and dichxylate compounds.
1 R A
[ s i ( O P ) J 301 34 l.M3,M7 100(1,2) x x x x x - - X
[si(CH3COJ3 ] 302"'Z"3" 90-95 x x x x x - - x (1 93-51
[si(CD3COa3] 3o2dgW - (1) O - - X - - - [Bi(02CCH2CH3)3] 3OJM1 lOO(2) - x x x x - - x
pi(OzCCH2CH2CH3)3 ] 304"' lOO(2) - x x x x x - x
[C(N&hI [Bi2WCM 32p2** x
[siO,hthd)(OH)] 321 '~ 97(11) - x - x - - - ** The original report codd not be obtained. Crystallo-bic infornation was extracted
f?om Chernicol Abstracts and the Cambridge Crystallogtaphic Database.
*Svntheses:
3.1) Bi203 + 6 RCOOH + 2 Bi(RCûO)3 + 3 H20
3.2) Bi(CH,COO), + 3 RCOOH + Bi(RC00)3 + 3 CH3COOH
3.3) %&O3 + 4 RCOOH + RC(O)OC(O)R + 2 Bi(RCOO), + 2 H20
3.4) Bi203 + 3 RC(O)OC(O)R + 2 Bî(RCOO)3
3.5) Bi(N0,)3eSH20 + 5 RC(O)OC(O)R + Bi(RCOO)3 + 7 RCOOH
+ 3 HNO,
3.6) BiCI, + 3 Ag-) + Bi(RC00h + 3 &Cl
3.7) NaBiO, + 2 RC(O)OC(O)R + N@i(RCOo),J + % 4 3.8) B i . & + 5 RCOOH + 2 L -B [H,LJ[Bi(RCOO)J + 3 P M
3.9) Bi(RCOO), + n L + RCOOH + Bi(RCOO),L, + RCOOH
3.10) Bi(RCOO), + HL + [Bi(RCOO)2(L)] + RCOOH
3.1 1) &O3 + 2 R(COOH), + 2 Bi {R(COO&)OH +
H, C2H9 C,H,, C4HJ9 were reportdy prepared by similar me?hods9 but are poorly
characterized. Pmliminary X-ray structural data was obtained for 319. An attempt to
prepare an O,O%iibe~lzoic acid analogue of [ B i M O H ) J 321 "' by a similar metbod
3.2.1 Catbonyiates
Bismuth foxmate Pi(OOCH),] 3 0 1 ~ ' ~ ~ ' shows monodentate fomate groups at
three different Bi-O distance ranges [avg. 2.38.2.52, and 2.77A 1, alI of which bridge to
neighbouring bismuth centers. The central bismuth atoms are nine-coordinate within
tricapped trigonal pnsms, which share basai tnanguiar faces and fomi a three-dimensional
network through bridging formate groups. Bismutho acctate [Bi(CH,COO), J 3 0 2 ~ ' ~ " ~
shows the bismuth center asymmetrically chelated by Uvce acetate groups pi -O 2.25(2)-
302
2.62(2)A]. Thrce oxygen atoms of two neighbouring complexes (O' and On; 0"') bridge
bismuth centers pi-O 2.8 l(2)-2.94( 1 )A] fonning a layemd structure and a nine-coordinate
environment for bismuth. Bismuth 2 J-dimethylpropioaate [Bi(02CCMe& J, 308Y'15' is
tetrameric in the solid state, with bismuth in a distorted nine coordinate environment. The
coordination sphere contains six ligands bound in various modes: monodentate and bndging
[avg. Bi-O 2.87-3.27A~; O,O'-chelating and non-bridging (avg. Bi-O 2.24 and 2.50Aj; and
0,Okhelating and bridging [avg. Bi-O 2.25-2.73A~. The tetramerie structure shows less
intermoIecular contacts than the threedimcnsional h e w o r k of the formate 301 or the
Iayered framework of the acetate 302, so that 308 is much more volatile at lower
temperatures In addition, the relatively pa ter thmal and hydrolytic stability of the
compound is accredited to the protection of the Rlaive sites by the buiky ligand.
@------Bi------
47 Bismuth benmate pi(C&C00),] 3 1 p shows a similar nine-cwrdinate
environment, however intemolecuiar contacts create a one-dimensional polyrner. The
bismuth center is asymmetricalîy chelated by three benzoate Ligands, fomiing four-
membered -BiOCO- rings. One oxygen atom of each ligand bridges to another bismuth
center pi-0- 2.198(14)-2.533(16); B i - 4 b , 2.243(14)-2.793(18)A] and in tum
each bismuth center meives a long contact ficm three Ligand oxygen atoms [Bi-O
2.624(l6)-~.380(16)AJ.
Neutra1 [Bi(CF3C00), J 31 1 monoanionic [NaBi(CF,COO),] 3 12~ ' and the
dianionic [H2teed]Pi(O2CCFJs] 3133n trifluornacetates have k e n prepared, as well as a
dianionic pentakis(f0nnate) cornplex K2[Bi(OOCH)5 J 3 14. '~ [Bi(CF,COû),] 3 1 1 is very
moisture sensitive, and a stnicture in which the three trifluoroacetate ligands are bound
monodentate to the bismuth atom is suggested based on i n h e d data However, high
melting points and IR data suggest significant molecular associations via bridging
tri fluoroacetate groups. The monomeric anion of 31 3 shows bismuth in a symmetnc ten
coordinate bonding environment, occupieû by five 0,O '-bidentate trifiuoroacetate groups
pi-O 2.44(3)-2.62(2)A]. The distorted pentagonai prismatic geometry can be simpli fied
48 to distorted trigonal bipyramidal if each carboxylate group is considenxi to occupy a single
coordination site. A similar ten coordinate structure is observed for 314.
The trifluoroacetic acid dduct [Bi(00CF3)3(HOOCF,)] 31S3" shows bismuth
bound to three asymmetricaily chelaîed 0,O'trifiuoroacetate groups pi-O, 2.26(3)-
2.27(3); Bi-O, 2.64(3)-2.9 1 (3)A], with the three shortcr Bi-O bond distances in a facial
arrangement, and a monodentate O-ûifluoroacetic acid ligand pi-O 2-71 (3)A]. A long Bi-
-O contact to and b m cach of two neighbouring molecules pi-O 2.79(3)-2.84(3)A]
creates a polymeric chah structure and gives an imgular nine coordinate geometry for
bismuth.
The thiourea adduct ~i,(CH3Cûû),COù,(H20)] 316'" is composed of dimenc
[Bi,(CH,COO), 1" anions and dimeric [Bi2(CH3COO)&) J2+ cations. The eight coordinate
bismuth center of the cation is bound by two bidentate acetate ligands mi-O 2.3 l(1)-
2.7 1 (2)A], three S-thiowea molecules [Bi4 2.677(5) and 3.1 ~ î (6 )A ] and a long thiourea
suifur contact h m a neighbouring group [Bi-S 2.909(5)A]. In the anion, bismuth is nine-
coordinate with four bidentate acetate oxygen groups [Bi-O 2.2~1)-2.78(1)A] and a long
acetate oxygen contact h m neighbouring monomer pi-O
(cation) (anion)
317
49 2.77(2)A]. The adduct pi(CH,C00)3@)3] 3 1 7 ~ ~ is composeâ of monomeric units, with
three 0,O'-bidentate acetate groups [avg. Bi-O 2.509(4)A] and th- fac thiourea d f u r
atoms [avg. Bi-S 3.06 1 (ZIA] in the bismuth coordination sphere. If each bidmtate acetate
group is considerrd to occupy one site, the ninecoordinate geometry may be reduced to
near octahedral.
In the dinuclear mixed a c e t a t e - u [1,3-bi~ethylarnin0)-2-propanolato]
complex ~ i ( 0 0 C C H 3 ) 2 ~ a ~ ) ] , [ H , 0 1 31en two bismuth atoms are bridged by the two
aminoalkoxide ligands p i - O 2.1 8(2)-2.4 l(2); Bi-N 2.68(2)-2.76(3)A]. In this instance, one
bismuth center is asymrnetrically chelated by two acetate Ligands [Bi-O 2.32(2)-2.91(3)A],
while the introduction of the water molecde [Bi-O 2.75(2)A] into the coordination sphere
of the second, and the monodentate bonding of an acetate gmup [Bi-O,, 2.48(2); Bi-O,
2.42(2) and 2.45(2)A], allows for retention of the eight coordinate environment for both
metal centers.
3.2.2 Dicarbo.qvZates
A comprehensive search of bismuth oxalate compounds unvcïled several
13o.3~9~60 nonhydrated and hydrated bismuth oxalate Pi,@zr)II6' and Bi2@LCh~nH,0
(n = 5,6, 7,'M3"8)3a]; ionic complexes [LiBi@a)pnH20 (n = 2, NaBim,*nH20
(NH,),Bi2(&F@2H20 and (NH,),~i,@rù~Cl@8~~0~~~]; complexes containhg fiee acid
[rn~i,(ox)~*nH~ox~~']; and a "sub"oxa1ate [(BiO)2@Ic)361]. There have been systematic
studies of the effect of the h2-y[Bi3"] ratio, sequeme of addition and st-g time on the
composition of precipitated bismuth oxaiate ptoducts h m aqueous solutions of Bi(N03)3
and H&', K a M 6 , (NH4)s367, N a 3 @ or Li92~.~'" Another solution study of oxalate
complexes involves the determination of stability and solubility constants of the
B i ( C 1 0 , ) 3 - N ~ - H 2 0 system by UV spectroseopy."' Fomulae assignments are typicdly
based on chernical analysis or thermal decomposition &ta.
The only cxystailographically characterized oxalate complex [C(NHJ,]~i,(pr)c13]
320Y2 shows bismuth in a nine-coordinate face cented trigond prismatic environment.
Bridging chlorine atoms form duneric units. A series of organobismuth dicarboxylates has
also been report& which includes the oxalate complex [PhBi@)], and was characterized
by EA and EI-MS.
5 1 The IR spectrum of [ B i w O H ) ] 321~~' indicam an ~symmetricai bidentate
coordination of both carboxylate gmups.
3.3 Results and Discussion
Crystals of bismuth oxalate octahydrate ~ i , ( ~ 0 J 3 ] * 8 H , O a were isolated in
very low yield fiom the reactions of excess oxaiic acid with either bismuth chlonde or
bismuth oxychioride in wata under reflux conditions. As with the syntheses of other
bismuth mono-and dicarboxylates, excess ligand is employed to minimize pH and
decrease the fonnation of insoluble hydrolysis products.
As is typical of bismuth carboxylates, the structure of a is highly coordinated,
with each oxalate ligand bonding in a tetradentate manner and bridging two neighbonng
bismuth atoms, as shown in Figure 3.1. Each of the two unique bismuth atoms is
chelated by three oxalate ligands [Bi-Owh, 2.33(1)-2.60(1)A] in a bidentate -0CCO-
fashion (favorable fiveaianbereâ rings). This is an unusual arrangement in that the
carboxylate functionality typically chelates in an -0CO- manner, but is similar to that of
320. Two water molecule oxygen atoms complete the coordination sphere pi-O,,
2.49(1)-2.~7(2)A], giving a total coordination number of eight. The Ione pair on bismuth
appean to be stereochemically active. The overail result is a complex the-dimensional
polymeric network, as observed for bismuth formate 301 and the
hydroxy/alkoxycarboxylates 20598 discusseâ in Chapter 2. There are four non-bonded
lattice water molecules.
The absence of chlorine in the isolated product is striking (cf.
[C(NHJ3][si,('gg)C13] 320'"). Chlonde ion bon& favorably to bismuth in solution and in
Figure 3.1 Crystallographic view of [Bi,(~0,),]~8H20 u. Selcçted bond leagths [A]:
5 3 the solid state, and is in excess in the preparation of a as shown in the following
proposed reaction quation sequence:
Attempts to isolate products nom reactions involving bismuth nitrate or bismuth oxide
were unsuccess hl. In teactions UivolWig bismuth c hlonde, generation of hydrochloric
acid during the reaction may allow for an effkctive decrease of pH below -1.3 (pK, of
oxalic acid), the approxirnate pH at which bismuth subnitrate crystals have been
i~olated,~' .~~*~' and a minimization of hydrolysis reactions. Also, the increased aqueous
solubility of Bi" in the presence of chloride anion (Chapter 2) may facilitate crystal
growth. The low yield of the isolated product precludes definitive conclusions regarding
the bulk reaction. Nevertheless, the isolation of the parent oxalate is an important
observation.
Interestingly, was also isolated in low yield h m the reaction of BiCI, with
excess glyoxylic acid afkr prolonged exposure to air. Aldehyda may be oxiâized to
carboxylic acids in the presence of mild oxidizing agents, such as Ag20 in basic media
(see equation 3-14)? In this case, the oxidizing agent is presumably 4, which is a
stronger oxidizing agent than BiO' unda acidic conditions (see equations 3.15 and 3.16,
respective1 y).'"
3.14) Ag,O + H,O + 2e- * 2 Ag + 2 OH- (EO M.342V)
3.15) 0, + 4 W + 4e- * 2H,O (EO +1.229V)
glyoxylic acid oxalic acid
Monocarboxylates (e.g. formate 301, acetate 302) have been prepared by
dissolving bismuth oxide in neat or concentrated acid (rraction 3. I ) . ~ ' ~ The liquid state
of these acids at room temperature allows for the essentiai absence of water and higher
isolated yields. Solid acids, such as oxalic acid, require the presence of water as a
reaction medium. This has been circumvented in the preparation of bismuth benzoate
310, which involves ligand exchange of bismuth acetate with molten benzoic acid (mp
1 22.4"C) with distillation of the acetic acid b y-product." High yields are also obtained
in the preparation of inorganic bismuth saîts h m concentrated strong inorganic acids due
to the high acidities (low pH) achieved.
3.4 Conclusions and Future Directions
The preliminary isolation of the parent bismuth oxalate from acid solutions
containing chloride anion illustrates a possible general synthetic route to the synthesis of
bismuth carboxylates. The acidic reaction conditions prevent the formation of polymenc
55 and insoluble bismuth hydrolysis products, while the presence of the chloride anion may
assist in preventing hydrolysis and solubilizing the Bi3+ cation.
Foremost to the continuation of this pmject is a comprehensive assessrnent into
the effect of pH and chlonde ion concentration on the formation of bismuth oxalate and
other dicarboxylates (e.g. rnalonic acià, diglycolic acid and thiodiglycolic acid). This
malonic acid E = O, diglycolic acid = S, thiodigylcolic acid
rnay be achieved through the addition of concentraîed hydrochionc and nitric acid in
various ratios. Lower pH conditions may facilitate the isolation of higha product yields,
while the presence of excess chlonde ion rnay promote the formation of various
chemically interesthg chlonde/carboxylate products. Further, cornparisons to reactions
involving monocarboxylates would provide insight into the importance of the chelate
ability of the ligand in product formation.
The polyprotic nature of lactic, malic and t a M c acids allows for the potential
isolation of a varie@ complexes with bismuth. However, few examples (one or two for
each ligand) have been structurally charactcrizeâ (see Chapta 2) and there have been no
systematic studies exploring sequentiai dcprotonation. Again, the efféet of reaction pH
conditions, Bi3' concentration and chioride ion concentration, as well as the chelate
ability of these hydroxy-carboxylate ligands, on product formation must be deterrnined.
Further, systems involving other medicinally relevant ligands such as salicylic, ciüic and
gallic acid must be examined.
56 In Iight of the prominence of the salicylate ligand in medicai applications of
bismuth, novel appmaches to investigating these complexes are of immense interest. An
alternative to the addition of excess mineral acid to UIcrease solution acidity, salicylic
acid may be derivatized to decrease its inherent pK value. This may be achieved through
the substitution of electron withdrawing groups on the ammatic ring, such as a nitro-
group in thepara position to the carboxylic acid fiinctionality (structure 1) or fluorination
of the aromatic ring (structure II).
Despite over 100 years of existence and rnedicinal utility, the structure of BSS has not yet
been detennined due to the insolubility of the compound. As of yet, only submicroscopic
size crystals have been obtained, which have insufficient dimensions for X-ray diffraction
studies. Three compounds closely related to BSS that have been structurally
charactenzed are bismuth "subnacetate 319," bismuth benzoate 310M and bismuth
thiosalicylate 548.'" however, only a preliminary structure was proposed for the
subacetate. Since the subacetate and the 4'sub"formate, p r q d in the same study,
remain the only bismuth "sub"carboxylates that have been crystallized, a comprehensive
reassessment of these preliminary results and a complete structurai characterization may
provide insight into the structures of this class of compounds and their relationship to the
structures of subnitrates, which also contain a labile anion. Further, the techniques
57 employed to prepare bismuth subacetatc could possibly be applied in prrparing crystals of
the "sub"salicylate, of sufficient size for crystailographic studies and stnictural
characterization. A similar approach may yield isolates of the medicinally relevant and as
of yet not structurally characterized "sub"gal1ate.
5 8 Chapter 4. Aminocarboxylates: New Investigations into the Bi-edta System
Iacluding Isolation of the Fint Cationlc Complcx
4.1 Introduction
H,edta is a strong chelator of most metals including bismuth, and the Bi-edta
system has been extensively studied in the solid state and superficially in solution. The
Bi-edta complex is an analogous polyciuboxylate system to the Bicitrate system and is
more soluble and rigid under various pH conditions, making it an excellent candidate
mode1 for the solution chemistry of CBS.
Polyaminoc~xylates, such as H&Q, are derivatives of a-amino acids, the
building blocks of proteins, and are themselves of biological interest. The cytoprotective
nature of commercial bismuth products is believed to Lie in the abiiity of bismuth to bond to
protein molecules of exposed tissuePa and any chemicai insight into bismuth-
aminocarboxylate systems is therefore of value.
This chapter introduces the established syntheses and structures of bismuth
polyarninocarboxylates, followed by the synthesis and structural characterization of the
first cationic Bi-edta species {Pi(Hedta)Jl,H) Cl.ZH,O a. A preliminary ESI-MS study
of the Bi-edta system, at low and high pH values, is also presented.
4.2 Synthesis and Structure of Bismuth-Aminocrirboxyiatcs
Several examples of bismuth polyambcadmxylatcs have been prepared, the
majority of which arc & complexes. and anploy ligands which possess wide variations in
chelate ability (i.e. number of fiuictional groups). Dcrivatization of more comrnon ligands
involves addition of a cyclohexyl ring to the hydrocarbou backbone (e.g. cvdma) or
substitution of acetate bgments for akoxyethyl p u p s (e.g- oedta). The water solubility
of bismuth polyaminocatboxylates increases with the nurnber of carboxylate groups on the
ligand, thereby facilitating crystai p w t h . However, fields are typically not reported and
studies are comrnoniy basd on single crystal X-ray difnaction studia only.
Characterizaion data for compounds discussed are contaiad in Table 4.1.
Bismuth polyaminocarboxylatcs arc typically prepareâ by heating under reflux a
suspension of a basic inorganic bismuth salt such as Bi,O, Bi(OH), or (BiO),CO, with the
appropriate ligand in water. Addition of base, such as guanidinium carbonate or an alkali
hydroxide, to the reaction mixture affiords the anionic salt in most cases. The neutral
dihydrated Pi(Hedta)(H,O)J 41 lmJX and non-hydrated3" complexes are reportedly
synthesized by analogous reactions involving bismuth subcarbonate and bismuth hydroxide,
respectively, while bismuth nitrilotriacetate dihydrate (Hm Pi&g&(H,O)J 4063753* and
the trihydrated produc?% are also isolateci h r n similar reactions. The trihydrated product
was characterized by elemental analysis and Uifirared spectroscopy only. The dihydrated
Table 4.1 Analytical data for arninocarboxylate compounds.
Compound yield X E 1 U N M T p (nui R A R V M S G o 4.n)* R A t
@~~(~I&(H~O)J 401358 80(1) - x x - - - - - ~i@&)(Hphç)@mso)] 402'" 42) x x - - - - -
~icondg)('H2O)J 403'" 40) x - - - - - O - [NHJ [si(Hond9),(HZo)3~ 4Wa 4-1 X - - - O - - -
~ C ( M I 3 3 l , [ s i ~ ~ 2 0 ) 3 1 4-1 x - - - - - - - 405~'''
60 Table 4.1 Analytical data for aminocarboxylate compouads (continued).
Compound yicld X E 1 U N M T p (nar R A R V M S G O 4.n)* R A t
B i w ( H 2 0 ) 2 ] 4M"' - (3,4) x x - - - - - - W,]JBiQ&J 4O1"lJ8' - (5) r - - - O O - -
~,]4~i(nta)2(NCS)].2H20 40%'~ - (6) X - - - - - - -
[Bi(Hoedta)(H20)] 40937sJu -(1) - x x x - x x
[ N a B i 0 ~ 2 0 ) . 1 41P' -(7) - x - x - x x
pi(Hedta)(H,O)J 41 1 384.385 -(3) x x x - - - - -
mi(H,O)d [si(edta)],.3H20 4 1 7 ~ ~ - (7) x - - - - - - -
~aBi(edta)(H,O), ] 41 - ( i l ) x x - - - X -
[NH41IBiCehtg)(~20)1 4193" -(12) x - - - - - - - [Bi(Hcvdta)(H20),] 420'" -(3) x x x - - - - -
[Bi(H2dtq)(H20)J 421 376.393 47 x x - X X - - (13,141
edta sodium salt ~ i ( e d t p c ~ ~ ~ 0 ) J ~ ~ ~ is reportedly prepared by adding an aqueous NaOH - solution to a suspension of (Bi(Hed@ J, though the compound has not bem
comprehensively characterized. The sodium [Bi(Na&p&@I,O),] 422376 and guanidinium
[C(NH33]2pi(&&(H20),] 423375 salts are preparcd h m the neutral complex 421, and the
high water solubility in cornparison to similar bismuth polycaTbOxy1ates is scmdited to its
anionic nature.
62 Complexes involving && have been most extensively c h a r a ~ t e r i z e d ~ ~ ' ~ ~ ~ and
ùiclude examples of both hydratedZmfu3-' and n~n-hydrated-~-~ pi(Hedta)], as well
as the ~&376.391.W1 K3* NH,:86Jw Mg,"'3 Ca,389" Sr, Ba, Ni, Zn, Cd,"'3 CO:^.*^ Cu" and
Mo3W salts of the pi(edta11- anion, as well as the potassium fluoride complex
several examples of [Bi(Hgdta)] (41 1-13) and pi(edta) J' (41 4-19} complexes.
Aminocarboxylate Ligands typically exhibit maximum chelation with bismuth,
forming five-mernbed -BiNCCN- and/or -BiNCCO- rings. The large covalent radius of
bismuth (1.52A) allows for chelation of Ligands in the bidentate to decadentate range.
Additional coordination sites are typically occupied by oxygen atoms of water molecules or
exocyclic carboxylate oxygen atoms of neighbouring molecules, creating polymenc
structures.
A structure containing three -BiNCCO- five-membered chelate rings has been
proposed for the quinaldic acid (H& complex [Bi@&(H20)J 4013" h m cornparison of
infhred spectra with previously characterized compounds.
The prndine-2,6-dicarboxylic acid (Hm complex [Bi@dçxHl&)(&nso)] 402"'
shows the bismuth center chelated by both an N'û-bidentate (Hmpdç) ligand and an OJV,O'-
tridentate 0'- ligand [Bi-O 2.209(8>2.507(6); Bi-N 2.4 l8(9) and 2.48 1 (9)Al. An O-
dmso molecuie in the remaining axial site mi-O 2.61(1)A] and a long cahxylate oxygen -
63 contact h m a neighbouring molecule [Bi-O 2.578(4)A] create a centrosymmetric dimeric
structure and a seven coordinate distorted pentagonaï bipyramidal geometry for bismuth.
The protonated carboxylate p u p p i -O ~.738(6)A] is not considered to be bonded to
bismuth.
In the neutraJ N-hydroxyethylnitrilodiacetic acid (H30ndq) complex
pi(onda)(HIO)J 40337g the unda)* ligand chelates bismuth in a teûadentate manner p i -N
2.49(2); Bi-0- 2.33(1) and 2.34(1); Bi-0- 2.1ql)Al. A long alkoxide oxygen
(O) contact h m a neighbouring moiecule creates dimers (Bi-O 2.46(1)A], which in turn
are linked by long carboxylate oxygm contacts of other dimers [Bi-O 2.7q1) and 2.98(1 )A]
to foxm a iayered structure. A water molecuie [Bi-O 2.77(2)A] completes the coordination
sphere and gives an eight coordinate distorted bicapped trigona1 prismatic geometry for
64 [C(NHJ3]2[si(~~&.pndgXH20)3] 40sJm also show the (HQ&)'- Ligand chelating in a
tetradentate fashion, despite the lowa basicity of the hydroxy- p u p in cornparison with
the alkoxide.
[Bi(pyg)(H20)J 406'" shows the bismuth center chelated in tetradentate fashion
by one m3- ligand [Bi-N 2.500(8); Bi-OeXyk 2.258(6)-2.253(7)A]. Two
intemolecular contacts pi-O 2.665(6) and 2.435(6)A] h m a neighbouring molecule
create a dimeric unit. The eight coordinate bicapped trigonal prismatic coordination
sphere is completed by the oxygen atorns of two water molecules [Bi-O,, 2.403(6),
2.767(9)A]. The monomeric anion of w,],[Biw4 40738'3" shows bismuth bound in
a tetradentate fashion by two m* ligands mi-N 2.58(1) and 2.60(2); Bi-O 2.44(1) and
B i-O 2.40( 1 )A], gïving a total coordination number of eight for bismuth and a doubly-
capped trigonal pnsm geometry. The structure of the b i s 0 thiocyanate compound
[(NH,),B i ~ , ( N C S ) ( H 2 0 ) J 408382 is andogous Fi-O 2.363(4)-2.5 5 1 (5); Bi-N
2.605(4)A], but also incorporates an N-isothiocyanate ligand mi-N 2.71(1)A] into the
bismuth coordination sphere, giving a nine-coordinate distorted tricapped trigonal pnsm
geometry at bismuth.
65 The whydn,yethylethyl~ediamine~acetic acid (H,oedta) compound
[si(Hoedta)(H,O)] 4w763U and the sodium sait ~aBi(oedt&(HZO),l 41v" have not been
Several bismuth complexes of ethylmediaminetetraacetic acid (H4edti3) have been
studied by X-ray methods~09384389J90*100-~**0i1 and al1 contain a hexadentate (Hedta)3-or
(edta)& ligand. The structure of pi(Hedt&(H20)J d l 13U38S shows the (Hedta]" ligand
[Bi-N 2.396(10) and 2.577(9); Bi-O 2.295(7)-2.7OO(l O)A]. The coordination sphere is
again completed by two carboxylate oxygen atoms of a neighbouring molecule pi---O
2.678(7)- 2.697(8)A], forming a dimer structure. The result is an eight coordinate
bicapped trigonal prism geometry for bismuth? The dehydrated analogue wi(Hedta)]
412"~ pi -N 2.465(5); Bi-O 2.399(3)-2.472(4)A] also shows two long oxygen contacts,
but fiom different neighbouring molecules [Bi--O 2.61 ~(s)AJ. This creates a one-
dimensional polymenc chah arrangement and a distorted square antipnsm geometry at
bismuth. The introduction of thiourea into the coordination sphere [Bi-S 3.03~(4)A] in
66 the adduct [Bi(Hedtg)&)J 413'" [Bi-N 2.5 lû(7); Bi-O 2.378(7) and 2.521 (9)A] prevents
intermolecular coordinations and results in a monomeric structure, bound ody through
hydrogen bonding.
In the [C(NHJ,]pi(edta)(H20)] 414'U anion, bismuth is similarly chelated in a
hexadentate fashion but by (edtaIC pi-N 2.56(1) and 2.59(2); Bi-O 2.34(1)-2.46(1)A].
A long Bi-O contact to and h m two separate neighbouring molecules pi-O
2.70(1)A] forms an &te anionic chain. A bound watcr molecule [Bi-O 2.69(1)A]
gives a total coordination numba of eight for bismuth and a distorted square antipnsm
geometry. nie calcium salt [Ca(H2O),][Bi&&)l2~2H2O 41sJa9 [Bi-N 2.460(6) and
2.543(6); Bi-O 2.360(6)-2.463(7)A] attains a similar polymeric chah structure, however,
the absence of the water molecule in the bismuth coordination sphm allows for a second
Bi---O long contact [Bi-O 2.778(6) and 3.038(ï)A] between monomers. Analogous
structures are observed for the isostruchual transition metal salts
[Co(HzO),] [si(edta)]p3H20 41 6 and [Ni(H,O), ][Bi(edta)]2a3H20 4 1 7.)" The sodium
salt VaBi(edta)(H,O),] 418'~' [Bi-N 2.495(5) and 2.508(5); Bi-O 2.3 IS(4)-2.521(4); Bi--
-0 2.636(4) and 2.850(7)A] and ammonium salt [NII,][Bi(cdta)(H20)] 419''~ [Bi-N
67 2.479(9) and 2.490( 10); Bi-O 2.290(9)-2.494(8); Bi-O 2.792(9) and 2.80~(8)A ] aiso
show two long Bi-O contacts h m two neighbouring monomers, but in these cases a
layered structure is created.
[Bi(Hc~dta)(H~O)~] 42v9 displays a simila. bonding situation to the edta analogue
414 pi -N 2.49 1(11 kî.5 1 3(lO); Bi-O 2.286(9)-2.497(11)& Long Bi-O contacts from
two neighbouring molecuies [Bi-O 2.6 1 2(9)-2.9 1 6( 1 0)A ] mate a polymeric network.
420 (Bi bonding environment)
[Bi(H,dtl,a)(H20)J 421)'~~~ shows the ( ~ d m a ) ~ Ligand chelating in a heptadentate
marner with one uncoordinateà acetate gmup p i -N 2.449(4)-2.723(4)A; Bi-O 2.290(3)-
2.699(3)A]. An eighth coordination site is occupieâ by a long Bi-O contact nom a
neighbouring molecule [Bi-O 2.620(3)A], giving rise to an infinite polymeric c h a i . and a
bicapped tngonal prism environment for bismuth. The guanidiniurn salt
[C(MI3J2Pi(d~a)(H20),] 423" shows that the ligand chelates in an octadentate
manner [Bi-N 2.536(7)-2.639(6); B i 9 2.368(~)-2.599(5)A 1. The coordination spbere is
cornpleted by an oxygen atom h m an adjacent molecule pi-O 2.686(6)A], creating a
dimeric structure and a nineccoordinaie monocappi squm antiprisn environment for
bismuth. The potassium salt [KBi(H&p&(HIO)s] 4 2 P shows a similar octadentate
chelating situation, but with a water oxygen atom completing the coordination sphere and a
monomenc structure.
in [C(NHd3 J2[Bi(cvdtpa) ] 425,'93 0% chelates in an octadentate manner [Bi-N
2.458(5)-2.592(5); Bi-O 2.371(4)-2.610(4)A] giving a monomeric structure. Here, bismuth
is in an eight coordinate environment, which may be daiveà h m a square antiprism.
425 (Bi bonding environment)
pi(H$tha3(H2O), ] 426" shows the (Hm3- ligand chelatuig in a ddentate
manner [Bi-N 2.472(8)2.8 1 3(8); Bi-O 2.320(7)-3.0~~(8)A]. The coordination geometxy
around bismuth may be descnbed as distorted bicapped square antiprism, with the two
extemai nitrogen atoms QU' and N') in capping positions. This is the fht example of a
426 427 (Bi bonding environment)
polyarninocarboxylate complex with coordination numôer ten. The bis(guanicîinium) salt
[ C ( N H J J J B i ( H O ) , ] 42y3* shows (HmE chelating in only a nonadentate manner,
wi th one noncoordinated carboxylic acid group (0') p i - N 2.6 19(7)-2.688(7); Bi-O
2.327(6)-2.560(6)A].
4.3 Results and Discussion
4.3.1 Synthetic Studies
H ydrogen bis(bisrnuth hydrogen N&flJv'-ethylenaiiamllietetraacetate) chloride
dihydrate {[Bi(Hgdt;i)J2H)CI@2H,0 a (Figure 4.1) is formed h m the stoichiometric
reaction of H,edta and b i s m u t h o chloride in water with addition of KOH. ïhe
isolation of the product h m reaction mixtures containhg 1-4 equivalents of KOH
demonstrates the favorabie crystdlization of this stnicture and the msistance of the Bi-
edta hexaadentate unit to small pH changes. However, reactions involving 0.5 and 5 - equivalents of base gave non-crystalline materials, which were not dennitively
Figure 4.1 Crystallographic view of {Pi(H&&H} C1*2H20 a.
7 1 charactenzed but were determined by Raman spectroscopy not to be the said product.
Reactions of bismuth subcarbonate t y p i d y yield the pi(H&t@] hydrated species, while
addition of a strong base such as guanidinim carbonate gives deprotonated anionic
species. The favorable crystallization of the cationic cornplex 46 is possibly a
consequence of the presence of the chioride anion.
The solid state structure of (see Figure 4.1) shows edta bonding to bismuth in
the familiar hexadentate manner. The absence of chlorine or water or long (Bi-O)
intermolecular contacts results in unusually low coordination number of six for bismuth.
Two neighboring Bi(Hedta)] units are bound at 0(6) to a common hydrogen atom
(proton). This hydrogen bonding phenornenon is characteristic of metal-
polyaminocarboxylate complexes and has bcen dubbed the "odd proton e f f e ~ t " , ~ with
two of the three examples of complexes involving ( H m L exhibiting this feature. In the
case of [Bi(Hedt@] 412 and the thiowa adduct 413,'" the "odd-proton" occupies an
inversion center and each molecule contains two "half-protonated" carboxylate groups,
resulting in the formation of hydrogen bound chahs. schematically represented by III.
The dihydrate 41 1 exhibits a specific location for the proton on a single carboxylate
group, which is hydrogen bound to a water molecule and terminates the system (see
diagram IV). For compound q& the odd-proton is located on a C, axis between two
Bi(Hedta) uni& without fiirther perpetuation, md a fblly pmtonatcd carboxylate group is
expected for each rnoiety of the cationic dinuclear unit (see diagram V), such as that
III IV
observed for 41 1.
X-ray crystallographic daîa suggests that the proton exclusive to each
mononuclear unit is bound at the exocyclic carboxylate oxygen O(2) and not the water
molecule, though this codd not be determincd with certainty. The C-O bond lengths may
be examined for clues to identify the remaining protonated p u p s (Table 4.2). For
[Bi-)(H,O)J 41 1,'"'" the position of the hydrogen atom was inferred nom the
equivaience of the carbon-oxygen bond distances of the three deprotonated carboxylate
groups, which is interpreted as conjugation of the double bond after deprotonation, and
the nonequivalence of those in the fourth carboxylate group. No such conjugation is
observed in 9& however, with the C-O bond distance discrepancy being -0.04A for three
carboxylate groups and -0.06A for the fourth [C(6) 1. Further, of the carboxylate groups
in question, bond distances suggest greater double bond character (Le. shorter bond
distances) for al1 exocyclic oxygen atoms. In both fi and 411 the bismuth center sits
asymmetncally in the O,N, cavity and is more closely bound to three carboxyl oxygen
atoms and one nitrogm atom. In the case of 41 1, the carboxylic acid group is tightly
bound to the bismuth center, and thmforc is not an indicator as to which group is
protonated. From a chernical standpoint, a hydmgen atom at 0(2) would allow for
hydrogen bonding of the chlorine atom to the ligand and is therefore a logical site for
the proton.
7 3 Table 4.2 Selected bond lengths for [Bi(H&&] complexes.
As discussed in Chaptm 2 and 3, the hydrolysis of Bi3+ to BiO' in al1 but strongly
acidic conditions typically deters the formation of soluble bismuth tris(carboxy1ates) in
aqueous media The significance of pK, in the preparation of arninocarboxylates has
been alluded to as the pretense for the failed isolation of a bismuth picolinic or dipicolinic
acid complex (i.e. pK, of -5 is too weak to react with bismuth subcarbonate), and in light
of the successfûl preparation of atê, edta and a complexes by similar methods.'"
However, the dipicolinic acid d m s ~ adduct 402 was successfilly prepared fiom the
reaction of the acid and Bi,03 in water, followed by fiirther reaction and recrystallization
of the resulting powder fiom hot ~. This suggests that reaction in &so is critical to
isolation of the product, and the absence of excess water at this stage may allow for
product formation. Further, the stmng Lewis base character of dm=, which foms
resilient complexes with bismuth, may aid in solvation of the ~ i ' + cation. Although
74 ligand pK, (pH of &on mixtures) does play a role, the strong chelate ability of
polyaminocarboxylates is most Uely the dominant factor in the formation and stability of
these compounds. The multidentate encapsulation of the bismuth center prevents
formation of the Biot bismuthyl ion in water. Thcrefore, bismuth complexes of bio-
relevant a-amino acids, which possess high pK, vaiues relative to monocarboxylates (9.6
for glycine venus 4.7 for acetic acid) and the ability for bidentate chelation only, may not
be prepared b m aqueous media Hydroxy-/alkoxycarboxylates, such as lactic, malic,
tartaric and citric (CBS) acids are much weaker chelators for bismuth and complexation
is expected to be much more sensitive to pH [e.g. citrate (CBS) requires an alkaline pH].
Only a small number of structures of this class of compound have been reported
exclusively within the past decade.
4.3.2 Preliminury Electrospray M a s Spectrometty Studies of the Bi-edtu System
Bismuth complexes are typically v a y insoluble and are subject to hydrolytic
reactions. Collection of solution data thmfore oAm requires sensitive techniques which
lend themselves to nonspecific experimental conditions. Aithough Bi-carboxylate
solution complexes have been examineci by a variety of physical and spectroscopie
techniques, none of these provide definitive formulae or structurai data Electrospray
mass spectrometry @SI-MS) involves the introduction of prc-fonned ions in solution into
the mass spectrometer. The subsquent scparation of ions accordhg to their mass to
charge ratio, as well as their controllcd fragmentation, provides ample information as to
the identity of solution species.
Bismuth complexes of citrate are complex in the solid state, while the
multidentate encapsulation of bismutth by & d o w s for the formation of simpler
pi(Hedtaj] and Pi(edta)Ja units. This, dong with the similar polycarboxylate structure
of the two ligands, highhghts the Bi-giQ system as a simple mode1 for studying the
solution chemistry of the Bititrate system and Bi-carboxylate systems in general.
Preliminary positive ion ESI-MS spectraa of the Bi-edta complex at low pH (1.4)
show peaks at mlz 499 (100% ml. htcii~ity) and m/z 293 (95% rel. intensity) assigned to
the [Bi(Hzedta)]' and [Hsedta]+ cationic species, respectively. At high pH (10.0), the
negative ion spectnim shows a peak at mlz 497 (100% rel. intensity) assigned to the
pi(edta)]- anion. These results contrast speculative conclusions based on
spectmphotometric and pH metric data that ouggcsts the decomposition of the complex to
the bismuthyl ion (Bi03 below pH 1.5 and the fornation of ~i(edtgKOH)]*- in the pH
range 8- 1 1 .'"
4.4 Conclusions and Future Directions
The strong chelate ability of polyaminocarboxylate ligands allows for the
formation of hydrolytically stable complexes with bismuth, while bifùnctional
aminocarboxylate ligands (e.g. glycine) p o s ~ s s insufficieut acidity or chelate ability to
deter hydrol ytic reactions. Investigation into scquential protonation of bismuth
polycarboxylates may provide fiirther insight into the significance of pH and chelate ability
on product formation. Further, prcliminary investigations demonstrate the inherent utility
of ESI-MS to study Bi-carboxylate systems in solution, which may be developed to
investigate the solution chernistry of CBS and other bismuth carboxylates and the
resilience of dirneric and polymeric associations observed in the solid state.
Reaction of a-amino acids with bismuth salts under anhydrous conditions would
eliminate the possibility for hydrolysis reactions associated with this system. This
method has been employed successfully in the synihesis of an organobismuth complex of
N-benzoylglycinate'"' and is a viable appmach to preparing other stable amino acid
complexes of bismuth?
As with the study of bismuth complexes of a-amino acids, investigations
involving di- and tripeptides would provide insight into bismuth-protein binding at ulcers
and throughout the body. Further, the variety of fiinctionalities associated with
polypeptides creates the potential for intmsting bonding situations. The only recent or
s igni ficant study that has been undertaken involves the tripeptide glutathione and
ranitidine bismuth citrate (RBC).~'* The thiolate (sulfhydryl) functionality was proposed
as the only site of binding by 'H NMR, but structural data could not be obtained.
Reaction of glutathione with simpler bismuth starting materials (e.g bismuth halides) in a
variety of pH conditions and solvents rnay allow for the isolation of chemically and
structural1 y interesthg produc ts.
The insolubility of bismuth subsalicylate has preveuted its structural
charactenzation to date, and the favorable hydrolysis of bismuth salicylate compounds
may be observed as a consequence of the weak chelate ability of the salicylate ion.
Derivatization of the ligand to include additional carboxylate gmups would incnase the
chelate ability of this ligand (cf polyaminocYboxylates), possibly allowing for the
formation of hydrolyticaliy resistant and soluble products. Potential avenues of
77 derivat ization include addition of carboxylate groups to the salicylate phmyl ring (e-g.
structure VI) or combination of two (e.g. structure WI) or more (e.g. stnicture WII)
carboxylate moieties:
Mn
As discussed in Chapter 2. the speciation of Bi3' in acidic media is still a matter of
debate."gs ESI-MS, which now has a demonstrated utility for Bi-ecita species in solution,
may also prove advantageous over previously ernployed methods (e-g
spectrophotometry. 209-2 13 and 2m21spotentiometicm7) in the definitive identification of both
positive ion and negative ion species prcformed in solution.
Cbnpter 5. In!roduction to Bismuth Thiolate Chembby
5.1 Introduction
The prominent thiophilicity (the preference to foxm bonds to sulfùr) of bismuth is
responsible for the facile formation of sulfido and thiolato complexes, which are well
established for most heavy metal elementsm niid atobismuth complexes represent the
most extensive class of B i 0 compounds for which a reliable set of data is available,
and include examples of monothiolates, dithiolates and bifunctional ligands incorporating
a thiolate group, as well as thio-substituted carboxylates. This chapter is provided as an
introduction to the synthetic and structural chemistry of bismuth thiolates and as a
background to the bihinctional thiolate chemistry discussed in Chapters 6 and 7 (for a
more detailed and generai overview of the structurai features for bismuth complexes
involving pnictogen and chalcogen donon see reference 410). A summary and
conclusions regarding the extensive data presented is provided in section S.S.
5.2 Monothiolates
Despite an extensive history, most examples of bismuth thiolates are poorly
charactenzed, with the f h t structurai studies of the more stable and soluble arythiolates
occwing within the past decade.'" Characterization data for bismuth-thiolate
compounds are catalogueci in Table 5.1.
Bismuth thiolates are typically prepared by reaction of the thiolate anion
(generated in situ) with a bismuth salt, however, the thiol will also react with bismuth
Table 5.1 Analytical chia for monothiolate compounds.
Compound yield X m E s 1 U N M T ( m 5 . n ) + R p A O R V M S G
1 R A Bi(SEt), 501'" - (1) - x - - - - - O -
Bi@%), 5024'3"'4 lOo(2) - x x 0 x - x x -
Bi(SCH,Ph), 5034'"4" 61 (3), 72 - x - - x x x - x (4)
Bi(SPh), 5044""'6 79(1) x x x x x - - - x
*Svntheses:
5.1) Bi(NO,), + 3 RSH + Bi(SR), + 3 HNO,
5.2) BiF, + 3 MqSiSR -* Bi(SR), + 3 MqSiF
5.3) BiCl, + 3 MSR + %i(SR), + 3 MC1
5.4) BiCl, + 3 RSH + NEt, + Bi(SR), + 3 NEt4Cl
5.5) Bi[N(SiMe& + 3 RSH + Bi(SR), + 3 m ( S M % ) z
5.6) BiPh, + 3 RSH + Bi(SR), + 3 PhH
5.7) &(SR), + L + Bi(SR),L
5.8) Bi(SR), + W(lB-crown-6)]SCN + [K(18-crownd)]~i(SR),NCS]
nitrate or triphenylbismuth to give the thiolate product. Other metathesis reactions
involve silylamine and silylsulfide reactants.
The pentafiuorinated aryl derivative Bi(SC$;), 51 24'6"'7"20 is prepared fiom the
reaction of the thiol with the bismuth cation in water or weakly acidic solution, or with
BiPh, under reflux conditions, while the reaction of BiCl, with three equivalents of the
thiolate results in the formation of the pentathiolate dianion ~a&f'),]~i(SC$,), ] 513,
instead of the tris(thio1ate) 512. The excessive thiolation of bismuth may be accredited ta
the increase in Lewis acidity of the bismuth centa resulting h m the electron withdrawing
influence of the fluorinated ligands. Additionaily, the greater nucloophilicity of the thiolate
overcomes the kinetic barrier.
The earliest reporteci bismuth thiolates arc those of simple akyl thiolates, such as
tris(ethylthio1ato)bismuth 501 :12 which are relatively rcactive compared to other bismuth
thiolates. Bi(S'Bu), 502 is stable under vacuum, but dccomposes in air and in
dichloromethane solution while Bi(SCH2Ph), 503 is îight smsitive."' Themolysis of
503 and the unsubstituted phenylthiolate compound Bi(SPh), 5044'5"'6 compound results
8 1 in the formation of bismuth metal, Bi& andlor disulfide~.~" The sterïcally encumbered
arylthiolate compounds Bi(SC&R',-2,4,6), 508-510~"*~" are air stable, sublime under
reduced pressures and are soluble in many organic solvents, while solutions oxidke to the
aryl disulfides.
The tns(alky1thiolate) Bi(S'Bu), 502 was determined to be monomdc in the gas
phase fiom mass spectrometry data, while its monomeric nature in the solid state is
inferred from cornparison of infrarrd data with that of the arsenic and antimony
analogues."'
The solubility of the unsubstituted tris(arylthio1ate) compound Bi(SPh), 504 4'5.4'6
in weakly donating organic solvents suggests a monomeric or weakly polymenc
structure, while preliminary X-ray analysis data suggest the compound has a similar
structure to 510.'16 The substituteà arylthiolate B ~ ( S C & B U , - ~ , ~ , ~ ) ~ 5 1 0 ~ " ~ ~ " shows
discrete monomers in the solid state, which is edorced by the steric buk of the ligand.
The bismuth center is in a three coordinate pyramidal environment [S-Bi-S 90.3(2)-
1 04.5(2)O] with identicai Bi-S bond distances mi-S 2.554(7)-2.569(8)A].
510
The pentafiuorinated aryl derivative Bi(SC&)3 512416-4'7~420 pi-S 2.532(2)-
2.584(2)A] shows a loosely bound dimeric unit in the solid state via a longer bndging
512 513
sulfûr contact pi-S, 3.323(2)A], with bismuth in a four coordinate disphenoidal
bonding environmat."" The dimerization of SlZ as compareci to 510 is presumably a
result of the l e s sterically bdky ligand. The structure of the anion [Bi(SC>J512- 513 shows
bismuth bonded to five pentafiuorothiolate ligands in a square pyramidal geometry Bi-
s,& 2.988(9). 2.703(9), 2.889(9) and î.W6(lO); Bi-S,, 2.609(10)A]. nie rernaining
apical site is occupied by a long intramolecular bismuth fluorine contact [Bi-F 2.94Al.
The incfeased Lewis acidity of the bisnuth center of 512 allows for preparation of a
number of Lewis base adducts [Bi(SC&(L) including examples of mono- (514 and
SIS), bis- (51 6-51 9) and tris- (520) adducts, and the anionic thiocyanate mono-adduct
~(I~-C~OWII-~)J~~(SC~~)~(NCS)] (521). AU structures are based on an octahedral
geomeûy and contain a pyramidal Bis, unit. A tram influence is observeci in al1 cases in
that introduction of Lewis base donors effects significantly longer Bi-S bond distances in
tram positions. The structure of mono- adduct 514 (L = SPPh,) shows the compound as a
centrosymmeeic dimer in the solid state, with bismuth in a five coordinate square
pyramidal geometry [Bi-Su 2.57(1)-2.62(2); Bi-S- 3 .O 1 (1)A] and involving a single
long contact h m a bridging suifur of the neighboring molccuie [Bi-S 3.1 S( 1 )A]. A
simila, structure is obsewcd for bismuth in the 521 anion [Bi(SC&),(NCS)]- pi-S,,
2.645(2), 2.2.6 14(2), 2.564(2)A]. in tbis case, the isottiiocyanate ligand bridges in an
-NCS- manner, and is more tightly held to the monomer through the nitmgen atom [Bi-N
2.577(6); Bi-S 3.178(2)A]. The bis- adducts 516518 (L = OPPh,, j m ~ a and DU>
respectively) show similar structures but are now monomeric [Bi-S- 2.548(2)-2.588(2);
Bi-SqM î.S74(2)-2.670( 1); Bi-O 2.502(3)-2.728(5); Bi-F,, 3.102(6)-3.254(7)A]. nie
structure of the tris- adduct 520 CL = SC(NHMe)J is similar to the bis- adducts, but
incorporates a third S-donor ligand into the maining axial site, creating a six cwrdinate
near octahedral environment for bismuth (Bi-S, 2.721(2); Bi-S, 2.946(3)A].
It is clear h m these structural obsavations that there is a tendency toward a
pyramidal facial arrangement for the Bis, unit of 512. Secondary bonding characteristics
are similar to that of the bismuth tribalides in the accommodation of one to three Lewis
base ligands, while the steric buk of the pcntafluorothioph~11olate ligand is s a c i e n t to
prevent the polymerization observed in mono- and bis- ligand complexes of bismuth
trihalides and phenyl dihaIidesYe6 These observai octahedral-based geometries and
84 tram effects are consistent with a mode1 involving B i4 a* acceptor orbitals, discussed
firîher in Chapter 7.3.
5.3 Bifunctional Thiolates
Several examples of bismuth complexes of bihctional ligands incorporating one
or two thiolate groups have been prepad. With the exception of the dithiolate species,
the increased solubility of these complexes (se Chapter 6) has allowed for more
extensive structural studies, particularly in the case of hydroxyethanethiolates.
Characterization data for these compounds is catalogued in Tables 5.2-5 .S.
Table 5.2 Analytical data for dithiolate compounds.
Compound yield X m E c 1 R M p (rxn5.n). R p A O R a S O
n m 1 [Bi (S(CHJ,S) CI] 52f"' 82(9) - x x - x x x -
522e2pyL12s 85(10) x x x - - - - -
[Bi {S(CHJ,S} Cl] 52J2 95(9) - x x - x x x - pi {S(CHJ4S) Cl] 524' 97(9) - x x - x x x -
[Bi {S(CH,)2S(CH~2S J CI] S2SL4- 87(9) r x x - x x x - [Bi {S(CH3,0(CH~,S}CI] 526Z4m 6@92(9) x x x - x x x -
{s(mJ~Ss) 31 527' 97(11) r x x - x x x - IB iz {S(CH2hS) 31 5282 92(11) - x x - x x x -
85 Table 5.2 Analytical data for dithiolatc compounds (continuai).
Compound yield X m E c I R M p (rxnS.n)* R p A O R a S O
~i2{S(CH~20(CH~2S)3]5312 99(11) - x x - x x x - mi {S(CHa2S} Br] ~ 3 2 ~ ' ~ %(9) - x x - x - - -
- -
~ 2 a 2 p r ~ ~ ~ 93(10) - x x - - - - - p i ( 3 ,4-S2CJr3Me)C1] ~ 3 3 ~ ~ ~ 84 (9) x x - - - - -
*Svntheses:
5.9) BiX, + HSRSH + Bi(SRS) + 2 HX
5.10) Bi(SRS)X + n L + [Bi(SRS)X]L,
5.1 1) 2 Bi(NO,), + 3HSRSH + Bi2(SRS)3 + 6 HNO,
5.12) m BiX3 + n NaSRSNa + s m ] C l + mJ,[Bi,(SRS)JJ + s NaCl
+ (3m-t) NaX
527 528 529 530 531
aqueous NaNQ solution. The sodium nitrate presumably promotes heterolytic Bi-Cl
bond cleavage, while the tethering illustrates the thermodynamic preference for the Bi-S
bond formation.
In addition to spectroscopie characterization, 522.2py. 525-27 and 530 and have
been crystallographically characterized and c o n h highly coordinated structures.
Compound 522.2~ shows bismuth in a sevm coordiaate distorted pentagonal
bipyramidal environment with the pyridinc donors in the axial positions pi-N 2.534(8)
and 2.592(9)A]. The equatoriai sites an occupied by two cir dithiolate sulfur atoms pi-S
8 8 2.545(4) and 2.592(9)A], an intermolecular sulfia contact pi-S 3.443(5)A], and two
nearly equivalently bound chlorine atoms [Bi-Cl3.111(4) and 3.23 1 (s)A], which bridge to
two separate bismuth centers and fom an alternathg Bi-CI polymeric backbone. The seven
coordinate environment of 525 (isostructural with 526) is occupied by a c h l o ~ e atom [Bi-
Cl 2.682(5)A], the two thiolate sulfvr atoms [Bi-S 2.541 (6)A], as well as a cross-ring
intramolecular donation b m the thioaher sulfur (ether oxygen for 526) [Bi4 2.849(5)A].
Iwo thiolate sulhu contacts Bi-S 3.534(*], and a long chlorine contact [Bi-Cl
3.285(6)A], nom a neighbouring molecule complete the coordination sphere. n i e tethered
bicyclic compounds 527 and 530 show similar iatramolecularly bound folded structures
with bismuth in six or seven u>ardinate cnvironments. Both compounds have similar
endocyclic Bi-S bond distances pi-S 2.~52(7)-2.599(4)A], while 530 shows slightly longer
cross-ring sulfùr contacts [Bi-S 3.07 l(5) and 3.197(4)A] than 525.
527 530
The anions [~i,(mntlJC,]~- and [B i ,bo lXJ2- 53641 are al1 speculated to be
dinuclear species, though no supporting data were obtained. The structure of the
tetraphenylarsonium salt I p h 4 A s ] p i m 2 J 543'*' shows a six coordinate bismuth center
chelated by two dithiolate ligands [Bi-S 2.664(7)-2.836(8)A]. Long sulfur contacts f~om
543
two adjacent molecules [Bi-S 3.238(10) and 3.182(10)A] create an infinite polymeric
chain.
5.3.2 Thiolatocatboxy~a~es
Table 5.3 Analytical &ta for thiolatocarboxylate compounds.
Compound yicld X m E 1 N M ( m 5 . n ) . R p A R M W
90 The few isolated examples of bismuth thiolatOcaTbOxylates have been prepated
similarly to both thiotates and carboxylates. Syntheses typically involve reaction of the
ligand with a basic bismuth salt or with the addition of base to ensure deprotonation of the
carboxylic acid group.
The infirared spectra of the tbioglycolic acid (mercaptoacetic acid, H a , 2-
mercaptopropionic (H22mna), 3-mercaptopropionic acid (Hdmna), and thiosalicylic acid
(H,tsd) complexes @i(L)(HL)] 5 4 4 4 y suggcst a polymeric structure, with bridging
mercaptocarboxylate Ligauds and four coordinate bismuth atoms.
H7&a w m W H.>3mDa H 2 W
A very complex octanuclear arrangement is observai for the ûis(thiosalicy1ate)
compound [{Bi,USaL),,~d~nf)~}(hf)~] 548;" With a C, symmetry and two unique bonding
situations for bismuth. One bismuth center (Bi') is chelated in an $0 (thiolate, carboxylate)
manner by t h e a ligands fonning six-membered -BiSCCCO- rings. The three sulfur
atoms are in afic arrangement [Bi-S 2.596(8)A] and al1 three oxygen atoms bridge to other
bismuth centers [Bi-O î.ï4(2)A]. The second unique bismuth center (Bi2) is chelated by
one ligand in an $0 manner [Bi-S 2.567(5)A; Bi-O 2.46(2)A] and two ligands in an
as-etrical 0,O ' manner [Bi-O 2.2~2)-2.79( 1)A] forming four-membered -Bioco-
rings. The oxygen atom of the S,O ligand and the more weakly bound oxygen atoms of
the 0,O '-w ligands bridge to neighbouring bismuth atoms. The coordination sphere is
completed by awoxygen atom Fi-0 2.60(2)A].
The unique trifiinctional aminothiolatocarboxyIate D-(-)-peniciilaminato-OJJV
compound [ B i w l ] 54gdM shows the Ligand chelating bismuth in a OSJI'manner
[Bi-O 2.414(5)A; Bi-S 2.527(2)A; Bi-N 2.345(6); Bi-Cl 2.680(2)A] forming botb a - BiSCCN- and a -BiOCCN- ring. Long contacts h m a chlorine atom [Bi-Cl 3.182A] and
two carbonyl oxygen atoms of neighbouring molecules [Bi-O 2.779(5) and 2.698(5)A]
create a polyrneric structure and a seva coordinate environment.
5.3.3 Hydroxy-/Alkoxy- and Ketothiobtes
Bifimctional thiolates incorporating a hydroxy- p u p have been extensively studied
and show a rich reaction chemistry. nie bis(hydrOxyethanethio1ate) compounds
[Bi(SCH,CH,OH)JJ (X = NO,^ Cl, Br) 550.52 are prepared h m the naaion of w o
92 equivalents of 2-mercaptoeulanol with the appropriate bismuth salt,' wwhile the perchlorate
sait (R = CIO4) 553,- is prepared h m a stoichiomeûic reaction in dilute perchlonc acid.
The impediment of maximum thiolation suggests some decrease in Lewis acidity of the
bismuth center. The reaction of bismuth retate with mercaptoethanol gives the alkoxy-
hydroxy complex [Bi(SCH2CH20)(SCH2CH20H}] 554.' in this case, aikoxide formation is
enforced by the basic character of the -te p u p s and may also be achieved from
Table 5.4 Analytical data for hydroxy-/alkoxy- and ketothiolates.
Compaund yield X m E s c 1 R U N M (mn R p A o o R a V M S 5.n)* 1 n m R
[ s i ( s C H 2 C ~ 0 ~ ( N 0 3 ) ( H , 0 ) , 1 41-76 r x x x x x x x x x 550'-"5 (17)
[Bi(SCH2CH20H)2Cl] 551' 73-78 x x x x - x x x x (17,181
[Bi(SCH,CH,0H)2Br] 552' 19-22 - x x x - x x - x x (17,181
pi(SCH2CH20Q(C104) 1 5S34x -(17) r x - x - x - - [si(SCH2CH20)(S~2cH20H)] 29-47 x x x x x x x - x -
5543.43s (1 920)
~i(SCH,CH20H)2(CH3COO)]5553 92(21) x x - x - x x - x x
[Bi(SCH2CH,0H),] 556'""' 33-70 X X X X - x x - (2223)
[si(&),] 557'" 69-90 X X X - x - (2425)
[BiPhCH @ 1 C W (0) Ph), 12 85-90 X - X X - X - [CH2ClJ 55tP9 (26)
[BiPhCH {SI C W (0) C~HIX)~] 85-90 X X - X - (X = Me, 559, Cl 5 6 0 ) ~ ~ ~ (26)
*Syntheses:
5.17) Bi& + 2 HSRH + Bi(SRH)J + 2 HX
5-18) Bi(SRH)& + MX' + Bi(SRH)JC + NaX
5.19) Bi& + 2 HSRH + Bi(SR)(SRH) + 3 HX
5.20) Bi(SRH),X + NaOH + Bi(SR)(SRH) + NaX + H Z 0
5.21) Bi(SR)(SRH) + HX + Bi(S-
5.22) Bi(SR)(SRH) + HSRH + Bi(SRH),
5.23) Bi(OEt), + 3 HSRH + Bi(SRH), + 3 EtOH
5.24) Bi203 + 6 HSR + 2 Bi(SR), + 3 H20
5.25) BiX, + 3 HL + NE4 + BiL, + 3 (HNEtJX
5.26) BiX, + 3 HSR + 3 NaOAc + Bi(SR), + 3 NaX + 3 HOAc
reaction of 550 in basic solution?* Recrystallization of 554 h m acetic acid reprotonates
the alkoxide and gives the acetate sait ~i (SCH2CH,0~(CH3C00)] 555.' Further, the
reaction of the hydroxythiolate-alkoxythiolate 554 with excess mercaptoethano143s also sees
reprotonation of the alkoxide and the formation of the tris(thio1ate) Pi(SCH2CH2OH),] 556.
Here, maximum thiolation is driva by the consequential fornation of the nucleophilic
thiolate group. The tris(thio1ate) bas also been prepared h m metathesis reactions between
mercaptoethanol and Bi(OEt),, and involves the favourable formation of etl~anol.'~' The
compound is stable under inert atmospheres but decomposes in air, contrasting the stability
of the bis(thio1ate) products. Compounds 551-52 may alsa be prepared by anion exchange
reactions with weakly bound nitrate p u p of 550.'
A11 bisfiydroxythiolate) structures show chelating hydrox y-/alkoxyethanethiolate
ligands, forming a bicyclic amangement of five-membcred BiSCCO- rings. The six
coordinate bismuth center of 550 contains a near planar hydroxyethanethiolate ligand
550 551 554 555
arrangement with cis sulfur atoms [ B i 4 2.639(5) and 2.655(5)& Bi-O 2.63(1)A], and a
bidentate nitrate group ( B i 9 3.01(2) and 3.17(2)A] bound above and beiow the Ligand
plane and adjacent to both hydroxy- oxygni atoms. The structure of 551 is polymeric with
bismuth in a seven coordinate environment [Bi-O 2.86(1) and 2.80(1); Bi-S 2.595(3) and
2.~58(4)A]. In this case, two /c,-chlori.ne atoms, which bridge bismuth to a second bismuth
center [Bi-Cl 2.589(3) and 3.488(4)A], and a long sulfur contact h m a third monomer [Bi-
-S 3.124(4)A] complete the coordination sphere. Compound 555 shows a monodentate
acetate oxygen atom [Bi-O 2.3~(2)A] and extensive hydrogen bonding [Bi-O 2.54(2) and
2.72(2); Bi-S 2.608(7) ami 2.577(7)A]. Preliminary structural data for 553 shows a simiiar
bis-chelating stmctwe with bndging thiolate suifur atoms [Bi* 2.61; Bi-S 2.97A~ to give
a polymeric arrangement. Compound 554 is polymeric and shows a five coordinate
bismuth atom, with the fiAh contact piovided by the aikoxide oxygen of a neighbo~g
rnolecule [Bi-O 2.982(8)A]. In this casê, the bis-chelating arrangemat [Bi-S 2.527(3) and
2.564(3)A] has one shorter and one longer oxygcn contact [Bi-O 2. M(9) vs. 2.577(9)A]
correspondllig to the alkoxy- and hydroxy- Bi-O contacts, respectively.
The ethexthiolate [Bi@&),] 557'' (Ha = 2,6irnethoxybenzenethiol) has been
characterized by elemental analysis and 'H NbfR only, although a crystalline material was
reported.
The structure of the ketothiolate [Bi(PhCH {S} C H F {O) Ph), J,[CH,ClJ 558"'
shows two unique bismuth centers chelated by thne ligands in an S,O manner, with a sulfbr
atom oecupying the axial site [avg. Bi-S 2.581(4)1j] and the remainllig atoms oecupying the
basal sites of the pentagonal pyramidal arrangement [Bi-S 2.627(5)-2.73 l(3); Bi-O
2.536(9)-2.650(9)A]. Long Bi-S' contacts [Bi-S 3.494(5) and 3.551(5)A] to the empty
apical sites between neighbouring molecules creates a dimeric stnichuc and a seven
coordinate bismuth center.
5.3.4 Amino-, Imino- and Aza-Thiolates
As discussed in Chapter 2.5, bismutho complexes of thioscmicarbazone
derivatives have been prepad as antimicmbid agents. Synthetic procedutes for these
compounds are general (reactions 5.27 and 5.29) and, due to the large number of complexes
isolated, oniy sûucturajly characterized exampies are discussed here.
96 Table 5.5 Analytical data for amino-, imino- and azathiolate compounds.
Compound yield X m E s c 1 R U N M p (rxn R p A o o R a V M S o
[S~(&R,R~(H&R,RJC~~]~~ SS(29 ) x x x - x x x x x - 569 (R, = C4H3S, R2 = C&)
[Bi(tscRlRJ2(N03)] 57VM 71(27) x x x - x x - x x x -
* Syntheses:
5.26) Bi(N03), + 3 RSH + n HCI + (3+n) KOH + Bi(SR), + 3 KNO,
+4H,O + n KCl
5.27) B i o , ) , + n RSH + Bi(SR)m(N03), + n HNO,
5.28) BiCl, + 2 NaSR + Bi(SRs1 + 2 NaCl
5.29) BiCl, + RSH + Bi(SR)C12 + HCl
5.30) BiCI, + HSRSH + NaN, + [Bi(SRS)N,] + 2HC1 + NaCl
The earliest aminothiolate bismuth compounds prepared were of
2-amuiobenzeaethiol (Hêbt)..YY4 The c o m p o d Bi- 561U) and the protonated
ammonium analogue Bi(H&),C13 562 are prepared similarly, with the d t i n g product
determineci by the tinal reaction p H . 561 is poorly soluble in organic solvents and
w4u appears to be air and moishm stable for a p e r d of weeks. The üis(thio1ate) compound
[si(2-SC,H,N-S-SiMe&] 564 is unstable to weak electrophiles (e.g. MC1 ), giving the
bismuth halide and the ~ u l f i d e . ~
For Bi(&& 561, participation of the amino- group in the binding of bisnuth is not
suggested by solid state IR, negating the presence of a chelating structure, while solution IR
spectra also suggests the presence of an uncoordinated NI& group. nie £ k t structurally
charac tenzed amino-thiolate [Bi(SCH,CH2NH~(N03~20)] 563"' shows a similar
bicyclic structure to the hydroxy-/alkoxythiolatts 550151 and 5-55, but with five-
membered -BiSCCN- rings [Bi-S 2.549(2) and ~.589(2)A]. Cooidination to the bismuth
center by a monodentate nitrate group and a water molecult gives a fomal coordination
number of six, while intemolecular contacts b m neighbouring sulfur atoms [Bi-S
3.5 1 7(2) and 3.550(2)A ] mate au eight co-ordinate distorted odahedral nivironment for
bismuth and a one-dimensional polymeric structure. The short bismuth-nitrogen [Bi-N
2.462(5) and 2.455(6)A] and long bismuth-oxygm [Bi-0,3.004(6)A; Bi-O,
3.107(6)A ] bond distances suggest an i n d stability for the bicyclic unit and decreased
Lewis acidity of the bismuth center.
Related to these aminothiolate complexes are those conbining ligands which
incorporate a nitrogen donor into an aromaîic ring. The tris(thio1ate) compound [Bi(2-
SC,H,N-3-SM%),] 564& has a distortcd pentagonal pyramidal geometry around bismuth
incorporating a pyramidal Bis, arrangement [Bi-S 2.544(6)-2.647(7); Bi-N 2.69(2)-
~.83(2)A]. The inverse relationship of the B i 4 and Bi-N bond distances suggests a greater
ring strain for the resulting four membered -BiSCN- rings than the -BiSCCN- rings of 563.
Bis(2-phenyl-8-mercaptoquinolinato) @me) bismuth chloride pi@&2C1] 56SU7
shows bismuth in a five coordinate distorted square pyramidal environment. The axial and
basal sulfùr atorns [Bi-S 2.532(3) and 2.591(3)A respectively] and the chlorine atom pi-CI
2.579(3)A] are in a fac arrangement, The long bismuth-nitmgen distances [Bi-N 2.628(9)
and 2.880(7)A] may be a consequeme of ring wPin enforced by the sp2 carbon backbone
atoms of the -BiSCCN- ~ g s , while the formation of the bis(thio1ate) is a possible
consequence of the induced decrease in Lewis acidity of the bismuth center by the imino
nitrogen donor, as well as the steric bulk of the ligand. A long sulfùr contact to the mpty
R = Me, ii-q = Ph, Hpmq
apical site [Bi-S 3.304(3)A] dimerizes the compound and increases the coordination
number of bismuth to six. The mlaîed trîs(methyi-) d o g u e [Bi(mmg),] shows
bismuth chelated by three 2-methyl-8-mercaptoquinoünate Ligands [Bi-S 2.571(2)-2.623(3);
Bi-N 2.689(4)-2.796(4)A] in afac arrangement with no intmolecular contacts, giving a
sixcoordinaîe distorted octahedral geometry for bismuth. A similar structure is observed
for the 3-mercapto- 1 ,Sdiphenylfomazan (dithizone) wmpound Bi(HPh), 56fu9 [Bi-
S 2.607(3)-2.6 13(3)A; Bi-N 2.678(8)-2.746(1 o)A], forming five membered -BiSCNN-
rings.
Examples of mono-, bis- and tris- complexes of various thiosemicarbazone
derivatives (H&çR,Ra have been prepared." The b i s 0 complexes [Bi(&R,R32(N0,)]
568 and ~ i ~ R I R ~ ( H & R I R ~ C I J 569 (RI = C,H,S, R, = C&3 bath show the & iigand
100 chelating in an Sa-manner, while in 569 [Bi-S, 2.527(3); Bi-N 2.5 1 S(8); Bi-CI 2.605(4)
and 2.630(4)A] one of the ligands bonds the bismuth =ter in a monohtate fashion as the
thione tautorner Bi-S, 2.992(3)A]. Compound 568 shows a similar bond arrangement to
568 569
the arninothiolate 563, with the a h c e of a bonded wata molecule [Bi-S 2.56 l(3) and
2.565(4); Bi-N 2.438(10) and 2.445(11); Bi-O 2.889(1 l)A]. The (RI = C,H,N, R, =
NCJ3,J derivatives [Bi&RlRJ2(N0,)J 570 and [Bi&R,R$lJ 571 both show the
Ligand chelating in a tridentate S,N,Wmanncr, forming -BiSCNN- and BSICCN- rings.
Compound 570 shows a monodentate nitrate anion and a seven coordinate environment for
bismuth [Bi-S 2.584(4) and 2.654(4); Bi-N, 2.471(8) and 2.581(8); Bi-N, 2.71 l(10) and
2.649(9); Bi-O 2.73 l(11 )A]. nie mono&& cornplex 571 dimcrizes via bndging chlorine
atoms, giving a total coordination number of six for bismuth pi-S 2.583(3); Bi-N,
2.355(8); Bi-N, 2.501(8); Bi-CI 2.585(3); Bi-Cl 2.791(3)A].
The 2,6-diacetylpyidine bis(thioJemicarbaz0ne) W2dabts) compound piCdants]N,]
572." shows bismuth in a six coordinate distortcd pentagonal pyramidal environment. Ail
572
basal sites are occupied by the SJV,N'JV",S'-pentadentate ligand [Bi-S 2.685(7) and
2.717(8); Bi-N, 2.46(2) and 2.58(2); Bi-N, 2.44(2)A~ with an azide nitrogen in the
apical site [Bi-N 2.25(2)AJ.
5.4 Thio- and DithiocarbosyIates
Bismuth thio- and dithiocarboxylates (Figure 1.1) are interesthg species in that they
may provide a usefiil link between thiolate chcmistry and carboxylate chernisby. The
thiophilicity of bismuth allows for the fomation of hydrolyticaily stable complexes, while
the group chelates and bridges bismuth in an d o g o u s manner to the carboxylate
functionality. While dithiocarboxylates have been extemively studied, t h m have been few
102 studies into thiocarboxylates of bismuth. The incorporation of both a hard oxygen atom and
a sofi sulfur atom or two sulhir atom gives way to structural divmity and allows for the
group to bond as a bihctionai ligand. As a result, examples of mono-, bis-, tris and
tetra(dithiocarboxy1ate) species, as well as mixed ligand complexes, have been prepared.
Characterization data for these compounds are included in Tables 5.65.7.
Table 5.6 Analytical data for thiocarboxylate compounds.
Compound yield X m E s I N (nai Sa)* R p A o R M
"Svntheses:
5.31) Bi@, + 6 RCOSH + 2 Bi(SOCR), + 3 H20
5.32) Bi(OOCCH,), + 3 RCOSH -B Bi(SOCR), + 3 CH3COOH
5.33) Bi(SPh), + 3 RCOSH + Bi(S0CRl3 + 3 PhSH
The series of tris(thiobenu,atcs) of the g a i d formula [Bi(SOCC$14R), ] 573-
75452.453 are themally stable, with 574 being much more soluble in orgaaic solvents than the
other derivatives. In 574, al1 three thiocarboxylate ligands chelaie to form four-mernbered -
BiSCO- rings pi -S 2.630(3)A], with quite long bismuth*xygen bond distances pi -O
1 O3 2.752(6)A] and the three sulfra atoms in a pyramidal /ac anangement. Long contacts from
the three sulfur atoms of a neighboring molecuie mi-S 3.498A] increases the coordination
number of bismuth to nine.
5.4.2 D W iocarboxyIates (Dithiocarbamates, Dithioxanthates)
The majority of dithiocarboxylate compounds that have been prepared are
dithiocarbamates 0, while thm are also several examples of dithioxanthates (Rdtx).
Both classes of compolmds exhibit a variety of organic R groups. &ed dithiocarbamate
compounds 51 10-117 include combinations of the following R (R') groups: Et, CH2Ph,
C,H,, C,H,, and C,H,-
104 Table 5.7 Analytical data for dithioçuboxylate compounds.
Compound yield X m E s c 1 U N M T C M (m5.n)* R p A O O R V M S G V W
IO5 Table 5.7 Analyticai &ta for dithiocarboxylate compounds (continuai).
Compound yield X m E s c I U N M T C M (m5.n)* R p A O O R V M S G V W
1 n R A [Bi(Et&), 1 5 1 0 3 ~ ' ~ ~ -(44) x x - x x x x x
[si(Tr&),] 51 û447u7""n -(u) ~ X - X - X - - - -
CsiOim31@ = c-call -(44) x - - - x - - - - - - 51 os, CHPh 5106)~'-.~"
[Si(EtrnA -(37,45) - - x - - x x - - - - x (X = Cl 5107, Br 5108)*'
[NEt,] [Bi(Etm4] 51 09*74*m - (46) x - x - x - - - - - -
IBi(&&&(R'2dlç)I 58-90 X X X - X X X X - x 5110-1 lys9 (47,443)
[Bi(Etdtx)2(Meg-Ù] 51 1- -(4Q x - - x x - - - -
[s i(R,dt~)~(Ettdgc) 58-97(48) - x x x - x x x x - - x (R =Et 5119; {CH,), 5120)
[si(Et&&Et&&J 5121" -(48) x - x x - - - -
[Bi(eac&J 5122&' gg,go x - - - - - - - - - - - (49,501
5vntheses:
5.34) BiC1, + 3 CS, + 3 NHR, + B i ( S 2 W 3 + 3 HCl
5.35) BiONO, + 3 HS,CR + (n+l) NH, + n HCI + Bi(S,CR), + H,O
+ NH4N03 + n NH,CI
5.36) BiC13 + 3 NH,(S2CR) + Bi(S,CR), + 3 NH,CI
5.37) Bi(S2CR), + X, + Bi(S2CQX + by-pT0duct.s
5.38) m Bi& + n Bi(S2CR), -+ (m+n) Bi(S,CR)),,&
5.39) BEI3 + 2 NH,(S2CR) + L + [Bi(S,cR)$I(L)] + 2 NKCI
5.40) Bi(S,C& + BF, + Bi(S2CR)z(BFJ + by-prducts
5.41) Bi(S2CR)X2 + L + [Bi&CR)J&)I + by-pducts
5.42) Bi(S2CR)12 + lrJEt4]X + (NEt4J[Bi(S2CR.)IA
* S vntheses: (continueci)
5.43) Bi(S2CR)Br2 + L + [HL]Pi@,CR),Br,,,J + by-pralucts
5.44) BiC13 + 3 Na(S,CR) 4 Bi(S2CR), + 3 NaCl
5.45) 2 Bi(S2CR), + C a , + 2 Bi(S2CR)J + Cu(S,ClQ
5.46) Bi(S,CR), + Nws2w + rNEt,llBi(S2CR)Il
5.47) Bi(S,CNR321 + CS2 + 2 + [Bi(S2CNRh(S2CNR'J
+ NHS2I
5.48) Bi(S2CR),X + M(S,CR') -, Pi(S,CRh(S,CR')I + MX
5.49) BiCI, + 3 HS,CR -P Bi(S,CR), + 3 HCl
5.50) BiOCl + 3 HS,CR + Bi(S,CR), + H 2 0 + HCl
Several methods have been uscd to prepare mono-, bis-, tris- and tetra- examples
of dithiocarbox y lates. These complexes exhibit varying degrees of solubility and
stability toward hydrolysis, oxidation and thexmolysis. The dithiocarbarnate [Bi(Et&&]
57645U56 is soluble in chloroform, carbon disulfide and carbon tetrachlonde, monorneric
in solution, and fairly air stable. The bis(dithiocarbamate) tetrafluoroborate salts
[Bi(R&),(BF,)] 590-92''' react with water, while the bis(dithioxanthate) halides
pi(Et&q (X = Cl 5107, Br 5108)'% are thennally stable but susceptible to hydrolysis.
Mixed-ligand complexes have also bcen synthesizeû, which incorporate two differnt
dithiocarbarnate or xanthate ligands, or both a dithiocarbamate and a dithioxanthate ligand.
These include mixed dithiocarbamate complexes [Bi(R&&(R'&) 1 51 1 ~ 1 1 7,'s9 a mixed
dithioxanthate complex pi(Et&&(Mc&Q] 51 18,- and mixed dithiocarbamate-
dithioxanthate complexes [ B i o @ u ] 51 l9 -12F and pi(Et&@t&.&J 51 21 .-
Compounds 51 l & l l 7 and 511P120 arc air and solution stable, while the mixed ligand
complexes 51 19-120 are more stable than tris(O-ethyldithioxanthate). An analogue of the
1 O7 2-ethylamino derivative complex [Bi(eac&] 5122&' involving the unsubstituted ligand is
reported without a formula designaion or characterization &ta.
There are several examples of tris(dithiocarbamate) compounds, al1 of which
contain three asymmehically S,S'-chelated ligands, forming four-membered -BiSCS-
rings. In each case, the shorter Bi-S contacts are in a fac arrangement, and varying
degrees of intermolecular Bi-S bonding create dimeric structures. The s t n r c t ~ r e ~ ~ ~ of
the diethyl analogue [Bi(&&&] 576'- [BiS2.595(5)-2.964<4)A] shows bismuth in a
seven coordinate environment, with a single long sulfur contact f?om a neighbouring
moiecuie p i - S 3.210(4)A~. The structure of the dieîhanol analogue
[Bi({HOCH,CH,)&), ] 5 7 y shows bismuth in an eight coordinate distorted square
antipnsm bonding environment [Bi-S 2.669(7)-2.885(7)A]. In this case, dimerization is
through four bridging sulfur atoms of two ligands [Bi-S 3.076(9)-3.179(9)A]. The
pyrrolidhe analogue Pi((CH,}&,] 5 7 p shows two unique bismuth atoms in both six
and seven coordinate mvironments [Bi-S 2.6 12(7)-3 .O l7(8)A 1. Here, only one of the
1 O8 bismuth centers receives a long Bi-S contact nom a ncighbouring molecule [Bi-S
A nurnber of bis(dithiocarbamate) halide wmplexes have also bem prepared and
conductance measurements of the bromo analogues [Bi(R&&Br] 579-83.66 suggest that
these compounds are non-electrolytes in nitrobenzene, while molecular weight
measurements of both the bromide and iodide analogues (Bi(R&,u 5 8 4 8 e 7 suggests
that they are b e r s in solution. Spectroscopic data for the iodo complexes suggest that
the dithiocarbarnate ligands function as bidentate ligands.
The bismuth centers of 579,584Im and 589- are each coordinated to two
asymrnetrically bound SJ'-dithiocarbamate ligands. Intemolecular halide and sulfur
contacts again ailow for varying degrces of polymerization. Compound 579 (NEC
omitted from drawing) shows tetramer-based polymeric network with two unique
bismuth environments. One bismuth center (Bi1) [Bi* 2.6~7(4)-2.843(7)A] coordinat es
two cis bndging fi- and fi-bromine atoms [Bi-S 3.066(2) and 3 . ~ 2 ) A . fe~pectively],
while a second bismuth center (Bi2) [Bi-S 2.641(5)-2.814(5)A] is cwrdinated to three fac
bridging h- and A-bromine atoms b: Bi-S 3.104(2); f i : Bi-S 3.232(2) and 3.390(3)A].
109 The structure of 584- shows a one-dimensional polymeric structure with a -Bi-1-Bi-1-
backbone, facilitateci by two cis bndging A-iodine atoms mi-1 3.257(2) and 3.3~4(1)A],
and bismuth in a six coordinate environment [Bi-S 2.646(4)-2.860(5)A]. The
bis(dithi0carbamate) thiourea adduct [Bi({CH2)&&C1(&)J 589."' shows bismuth in a
seven coordinate environment Pi-S* 2.624(4)-2.805(3)A; Bi-S,, 3 .O 1 7(4)A 1. A
dimenc structure is fomed through two cis p&lorine atoms [Bi-Cl 2.9 1 l(4) and
3.187(4)A].
Conductivity data for the tetrafluoroborate saits [Bi(R&&(BF,)] 590-92'''
suggest that the compounds are univalent-electrolytes in nitrobmzme, while molecular
weight measurements in dichloromethane suggests the compounds are monomerïc in
solution.
Examples of mono(dithiothiocarbamate) dihalides have also been prepared. The
ethyl denvatives [Bi(Et&)X,] 593m*4a'-954m a2are isostructural and show a one-
dimensional polymer with bismuth in a seven coordinate envir~ment.'~' The
110 coordination spheres are occupied by an S,Sdithiocarbamate ligand pi-S 2.594(3)-
2.690(5)A], two pairs of cis &-halogen atoms which bridge to two neighbouring bismuth
centea [Bi-X: Cl 2.673(3)-3.165(3); Br 2.820(2)-3.305(2); 1 3.032(2) and 3.~01(2)A],
and a bndging sulhrr atom fiom a neighboring molenile pi-S 3.378(3)-3.462(5)A].
The intermediate mono-/bis- complexes of empirical formula
[Bi,(Et&&X,(dmn] 596-98"' are also isostructural aad show a pentanuclear unit with
two six and one seven coordinate unique bismuth cnvironments. One bismuth atom (Bi')
is coordinated by two SJLdithiocarbamate Ligands Bi-S 2.6q 1 )-2.8 1 (1 )A], a terminal
halogen atom pi-X: Cl 2.89(1); Br 3.050(2); 1 3.278(3)A~, a bndging fi-halogen atom
[Bi-X: Cl 3.42(1); Br 3.5 15(3); 1 3.706(4)A], and a bridging ,u3-halogen atorn pi -X: Cl
3.43(1); Br 3.533(3); 1 3.680(3)A]. A second bismuth center (Bi2) is in a similar bonding
environment pi-S 2.61(1)- 2.8ql)A; Bi*-X): Cl 3.04(1); Br 3.194(3); 1 3.42 1 (4)A; Bi-
@,-X): CI 3.42(1); Br 3.469(3); 1 3.582(3)A], but with the absence of the temiinal
halogen atom. A third bismuth center (Bi3) is coordinated to bndging &-halogen atoms
[Bi-X: Cl 2.68(1) and 2.74(1); Br 2.860(3) and 2.862(3); 1 3.07q3) and 3.053(3)A] and
p3-haiogen atoms pi-X: Cl 2.71(1); Br 2.855(2); 1 3.079(3)A] only.
Several anionic complexes have also bccn prcparcd, including the monoanionic
compiex ~ t , J ~ i ( E t g f ç ) 1 3 ] 599 and the partially brominated [NEt,][Bi(Et&&Br]
11 1 5100:n and the dianion [HPY],[Bi,(Et&&Br,,] 5101 ."' The dimeric anions of 599 and
5100 are isosûuctural and show bismuth in a six coordinate distorted octahedral
environment. In addition to the S,S'-dithiocarbamate ligand [Bi-S 2.649(5)-2.770(6)A],
the bismuth coordination sphere is occupied by axial and equatoriai terminal halogen
599-51 00 5101
atoms [599: Bi-1 2.965(1) and 3.091(1); 5100: Bi-Br 2.813(2)A and Bi-1 3.006(2)A] and
axial and equatorial bridging iodine atoms pi-1 599: 3.190(1), 3.29 l(1); 5100: 3.1 15(2),
3.244(2)A]. The anion of 5101 shows a tetranuclear unit with bismuth in a six coordinate
environment. The coordination sphere contains one tenninal [avg. Bi-Br 2.94(1)A] and
three bridging bromine atoms [Bi-Br 3.24( 1 )-3 .34(l )A], and an S,S'-dithiocarbamate
ligand [Bi-S 2.68(3)-2.73(3)A]. Therc is aiso one very long contact to the empty site on
each bismuth center [avg. Bi-Br 3.74( 1 )A].
A number of dithioxanthates have Ptso been prepared, Uicluding the tris- products
[Bi(R-),] 5102-106,"~'~ and have structures similar to the tris(dithiocarbarnate)
analogues. Conductivity measurerncnts suggest that the ethyl derivative pi(Eth-L),J 5103
dissociates in ethanol solution The structure of [B~(MC&)~] 5102'~ pi-S 2.5%(3)-
2.998(4)A] shows a dimeric unit anaiogous to [Bi(Et&&] 576, where the mcipmcation of
a long ~ i - s contact pi-S 3.405(1)A] h m a ncighbouriag molede creates a dimeric
arrangement. The c yclohexyl- and knzyl- analogues 51 05 [Bi-S 2.599(2)-3 .O63(2); B i 4
112 3.21qî)A] and 5106 [Bi-S 2.597(1>3.025(1); B i 4 3.375(1)A] have analogous
stru~tures.~~ The one-dimensional polymeric anangement of ~ 1 0 3 ~ ~ [Bi-S 2.605(8)-
2.99(1 )A] involves two long suifur contacts h m two neighbouring molecules Bi-S
3.3 52(8)-3.627(9)A], giving a bismuth-dfk "1addei'-type pol ymeric backbone. The
5103 5104
structure of pi(?%,&&,] 5104475*478 is similar to that of 5102, but in this case the long
bismuth sulfur contacts of the molecular unit are to two separate neighbouring molecuIes,
fonning a one-dimensional coordination polper [Bi4 2.682(2)-3.175(2); Bi--S
2.842(2)A].
Spectmscopic data of the bis(dithi0xanthate) haiides [Bi@- (X = Cl 5107, Br
51 08)"~ suggests solid state polyrneric structures, while molecuiar weight measurements
suggest that they are monomeric in solution.
The monomeric anion of the teîzakis(dithioxanthate) w, J [Bi(Etm4] 51 0g4"
shows an eight coordinate bismuth center bound by three asymmetrically bound [Bi-S
2.803(11)-2.972(10)A] and one syrnmetrically bound pi-S 2.833(6) and 2.859(9)A] S,S-
113 dithioxanthate ligand?
Although there are no examples of stnicturaîly characterized dithioczubarnate and
dthioxanthate rnixed ligand complexes, infraied data for (Bi(R#tc),(EtpqO] 51 19-1 2 0 ~ ' ~ and
[Bi(Et&)(Et&&J 5121- suggest that dithiocarbamate ligands are more strongly bound
than dithioxanthate ligands due to 2-SS,C=W resonance.
in addition to the dithiocarbamate and dithioxanthates, 2-aminocyclopent-1 -ene- 1 -
dithiocarboxylic acid (Ha derivatives have ken cmployed as iigands for bismuth. The
2-ethylamino derivative complex Pi(eacd)J 5122*' shows a six coordinate distorted
R = H , H a R = Et, Hgacd
trigonal antiprismatic environment for bismuth, with three asymmetrically bound S , S
dithiocarboxylate ligands [Bi-S 2.617(2 )-3.108(2)A]. A long bismuth Julfur contact [Bi-S
3.689A] creata a weakly bound dimaic structure similar to 576.
5.5 Summary and Conclusions
In surnmaq, the data for bismuth-thiolate compounds presented in this chapter
(see Figure 5.1) is intended as an introduction to the synthetic and structural chemistry of
bismuth thiolates and as a platform for discussions regarding bifunctional thiolate
chemistry in Chapters 6 and 7. For the most part, the database for the thiolate chemistry
of bismuth is extensive, but is composed of examples which represent unique complexes
114 for a particular Ligand, rather than M e s of rclatcd compounds establishing fiuidamental
synthetic guideluies and illustrating g e n d chernical properties. For monothiolate ligand
complexes, the high thiophilicity of bismuth routinely imposes multithiolation and results
in tris- thiolation in mort cases. The introduction of an electmn-withdrawing fluorinated R
group increases the Lewis acidity of the bismuth centter and facilitates the isolation of
S"E \ C E-Bi-S
/ / \ \ R-S E-R
Figure 5.1 Bonding situations observeâ for bismuth thiolate complexes.
pentathiolate dianion and a series of Lewis base adducts, al1 of which exhibit octahedral-
based geometries. The thiophilicity of bismuth is huther demonstrated by the foxmation
of highly coordinated and stable monocyclic bis(thio1ate) and "tethered" üis(thio1ate)
complexes from dithiolate ligands. Few bismuth thiolatocarboxylate complexes have
been prepared and show the ligand chelaîing bismuth in both $0 and 0,0 capacities,
result ing in extensive intermolecular bonding typical of the carboxylate huictionality .
Although there are tris(thiolate) examples of complexes incorporating bihctional
115 ketone-, imino- and azathiolate Ligands, the introduction of secondary electrondonating
fùnctionalities ailows for a potential dccrta~e in Lewis acidity for bismuth and control of
thiolation. This is demonstrated by the preference for a bicydic bigthiolate) arrangement
of bismuth hydroxy- and amino-ethanethiolates, as well as the isolation of bis- and
rnonothiolate complexes of the thiosemicarbamne ligand. Mono- and dithiocarboxylates
chelate and intermolecularly bond with bismuth analogously to the carboxylate
firnctionality, and may be viewed as bifhctional thiolatts, incorporating a secondary
ketone or thione donor. Oaly triS(monothiocarboxylate) complexes have been reported,
while dithiocarboxylates cmently represent the most varied coordination number for
bismuth with examples of mono-, bis-, tris- and tetra- complexes known, but involve a
range of ligands and a variety of synthetic procedures.
116 Chapter 6. DeCining and ControUg the Aminatbanethiolate Cbemistry of
Bismuth(III): Synthesb and Comprchcnsive Cbaracterization of Homologous
Thiolatobismuth Series
6.1 Introduction
Difficulties associated with isolation and characterisation of bismuth compounds
have precluded comprehensive assasment of their relative stability. Isolation yields are
oAen not reported or are low, and are rarely evaluated in t m of other possible reaction
products. Nevertheless, the synthuis and chemisûy of these compounds remains
superficially understood in that most compounds have been isolateci under specific
conditions and without investigation of other possible reaction products. Moreover, there
are few exarnple~~"~ of studies hto the repmducible interchange between derivatives or
related compounds, and variation in antimicrobial bioa~tivity'""'~ among the members of
systematic senes of structurally simple compoundsU suggests a stnicture/activity
relationship for the bismuth envkonment.' Such realizations highiight the need for
universally applicable synthetic procedures which enable control of the coordination
chemistry for heavy elements. Comprehensivt structural and spectroscopie
characterisation of systematic series of compounds represents the most reliable
fundamental foundation for rational chernical development.
The potential utility of chelating bifunctional ligands, containhg one thiolate
moiety and an auxiliary donor to mediate the thiophilicity of bismuth is demonstrated by
isolation of the bicyclic bis~ydroxyethanethi01ato)bismuth complexes 55041,553 and
5553,4~~,436 as most readily isolatcd products.'" Further, the andogous
117
bis(aminoethanethio1ato) bismuth nitrate compla 563 [hereafter denoted ~(N03).H,0]
is the oniy reported product of the reaction between Bi(NO,), and aminoethanethi01 in
acetic acid."' The penicillarnine compound 549 represents a unique example of a
mono(thiolate), but is facilitated through the introduction of an anionic carboxylate
fun~tionality.'~
in addition to the examples presented in Chapter 5 (561-63), there are rare examples
of spaîmscopicaily characterized oqpobismuth aminobenzenethiolate @J& complexes.
The preparation of both the mono- and bis(thio1ate) compounds [BiPh,(&)lU7 and
piPh(abtt)JW3 h m Hg& and BiPh, represent the only reports of variable thiolation h m
common starting materials. However, it is odd that the formation of the monothiolate
product involves a greater stoichiometry of thiol reactant [l : 1 vs. excess BiPh, for the
bis(thio1ate)J and heating, both conditions which would be expected to promote maximum
metathesis. The methyl bis(thio1ate) analogue [ ~ i ~ e ( â b t M F and a series of dimethyl
thiolate compounds Me$3iSRa were R is a nitrogen substituteû organic ring, are prepared
fiom metathesis reactions involving allrali metal thiolates and organobismuth haiides.
To exploit the realization of variable and minimal thiolate coordination, a
comprehensive assessrnent of the reactions involving BiCl, or Bi(NO,), with
arninoethanethiol or dimethylaminoethanethiol was perfomed at various stoichiometries,
in the presence of KOH. Addition of base serves to activate the thiol (to a thiolate), and
thereby provides a reliable and direct control of the extcnt of metathesis. in this manner,
this chapter defines the conditions to preparc and characterize homologous series of tris-
0, bis- and rnono(anilnoethanethiolato)bi~~~luth complexes = and d~). and
the solid state structure of at least one example of each has been confhed, thereby
118 clarifying and expanding the lixnited p r e h b a q conclusions arising h m previous
spectroscopie 4 ~ . 1 « ) . ~ I.w,us.~w.~~ I and structural studies.'"*us
6.2 Results and Discussion
The aminoethanethiolate and dimethylaminoethanethiolate anions react rapidly
with BiC!, or Bi(NO,), to give yellow solutions h m which crystalline materials have
been isolated by various solution concentrathg procedures. Isolates fiom reactions of the
dimethylaminoethanethiolate anion with BiCl, reflect the respective reaction
stoichiometry [3 : 1 gives Ume), 2: 1 gives m(Me), 1 : 1 gives m e ) ! . In contrast, tris-
thiolation to give a can only be achieved with the parent aminoethanethiolate ligand by
introducing a heavy excess (5: 1) of the anionic ligand, and the precise 3: 1 stoichiometry
affords =Cl.
R = H for compounds labeled @!! R = Me for compounds labeled Uwe)
The apparent impedance of complete metathesis for the parent ligand is likely due to
coordinative interactions nom the pendant amina, which inevitably mediate the Lewis
119 acidity of the bismuth center. The apparent weaker donor ability of the dimethylamino-
functionality @& of NMG 4.13) over that of the amino- group (pK, of NH2Me 3.35) is
counterintuitive and is accredited to the relative increase in steric restrictions, as observed
in the methylated (amine) derivative m(Me)CI]. Also, the excess Ligand is anomalously
soluble in the reaction mixture to give and mC1 shows an enhanced solubility in the
presence of excess ligand. This may be interpreted as indications of the incipient
formation of anionic poly-thiolates of the type [Bi(SCH2CH,NRJ, 1- and
[BiX(SCH,CH2NR&]', respectively, the lability of which may be reqmnsible for the
broad signals observed in NMR spectra (vide infra), and the existence of which
contributes to the incompleteness of thiolation.
Reactions involving Bi(N03), with the methylated ligand typically give oils on
evaporation of solvent, so that m(Me)NO, and &(Me)N03 have not been isolated, and
an insignificant yield of a ( M e ) (identified by Raman spectroscopy) was obtained from a
3: 1 reaction stoichiometry. Further, the lability of the nitrate co~ntenon'~ suggests that
the monothiolate compound 6ç(Me)N03 is not likely to be isolated. Nevertheless, the
parent compound m N 0 , is d l y obtained both as the previously reported hydratai
f ~ r m , ~ ' and as an unsolvated solid. The forma is isolated h m relatively dilute solutions
containing excess ligand (3: 1 stoichiomehy), by slow crystal growth over a number of
days. Rapid crystal growth h m preconcnitrated solutions of appropriate stoichiometry
give @NO3. Thee synthetic routes may be viewed as improvements over the iiterature
preparation,us which could not be repeated despite several attempts and of which the
original reaction conditions an questionable. The naftion involves similar reactants but
is performed in acidic media, and would be expccted to give ammonium salts.
120 Reactions of BiX, with dimethylaminoethauethiol or dimethyIaminoethanethio1
hydrohalide give m(Me)X (X = CI, Br) as an essentially quantitative precipitate,
independent of stoichi~rnetry.'~~ This dramatic thermodynamic preference for
coordination of the ammoniwnethanethiolate tautomer of the thiol is confirmed by the
high yield substitution of nitrate for chloride/ bromide observed in the 3: 1 reaction of
HSCH,CH,NMepHX with Bi(NO,),. Moreover, precipitate mixtures containing
6CWe)CI and KCl produce m(Me)Cl when washed with water, illustrating the labile - and basic nature of the amine chelate interaction.
Except in the case of de(Me)X [obtained as a analytically pure powder in 97 (Cl)
and >95% (Br) yield], the isolated yields do not generally illustrate quantitative reactions,
that are sometimes observeci for thiolate-bismuth systems,' and each reaction mixture
may contain al1 of the metathetical products that have been iso1ated over the range of
stoichiometric conditions. Nevertheless, it is clear that the imposeci stoichiometries
conveniently and sufficiently enhance formation of one complex over the others to allow
for isolation by crystal growth. Compound dç(Me).'/rHCl is reproducibly obtained
(each sample characterized by X-ray crystdlographic analysis) as Pasteur isolated
crystals from a powder mixture.
Bismuth thiolates typicaily exhibit low solubilities in most solvents and strong
donor solvents are required to enable any appreciable solvation, usually with the
formation of a resilient solvent coordination compIex (tg. S22m2~y, 5 3 2 . 2 ~ and
533 ."21"32 Complexes involving the bifûnctional chelate ligands
aminoethanthiolate and hydroxyethanethiolate have substantiaily higher mlubility,
121 perhaps due to the presmce of the awiiiary donor site on the ligand, which mimics the
role of the donor solvent and occupits possible intermolecular coordination sites. As a
result, these complexes an more routinely tecrystallised and are amenable to solution
NMR spectroscopie characterization. 'H and "C NMR spectra are consistent with the
compounds retaining theu topological solid state structures in solution, but signals are
generally broad, implicating exchange processcs, possibly due to the formation of
hypervalmt anionic complexes and consequential ligand lability.
As is typical for thiolatobismuth compounds, these complexes are thennaily
sensitive and, except for compound fi and W e ) , al1 decompose (dramatic color
change) before melting. Each compound exhibits a number of usehl features in the IR
spectra, but the Raman spectra show very distinctive and intense bands below 400 cm-',
which can be conveniently used as a reliable "thgerprint" identification of crystalline or
powder matenals.
While electron impact mass spectra of thiobismuth compounds are generally
uninformative as a result of their t h e d instability, the APCI technique3 provides
characteristic fragments, the most prominent of which are the bis-thiolates and
6B(Me)' ( m h 361.41 7), and atomic bismuth (rnh 209). Other fragments include the - bismutheniurn monocycle @i([email protected])]' (m/z 284), ~ i ( S ~ H , N H ~ C I J t (m/z 320) and
[Bi(SGH,NH&l+ (PmD3* (mh 393) for wl and [Bi(SC,H4NMi)Cl)+ (m/z 348) for
6B(Me)CI. A protonated molecular ion is also readily obscrved for m(Me)CI (m/z 453) - and m e ) (m/z 384). In addition to otha fiagrnents also observed for U m e ) and
6B(Me), spectra of both compounds show a solvent adduct peak [Bi(SC2H,NMwl + -
122 (dm fi]' (mk 42 1). interestingly, m(Me)Cl displays the m/z 4 1 7 ihgment, suggesting
that ligand lability allows for rearrangement to a bicyclic configuration.
The solid state structures of compounds 6& W e ) , m,, aNo30H20, =Cl,
6B(Me)CI, s(Me)*'/rHCl and m(Me)Cl have been confinned by X-ray crystallography -
(Table 6. l), although the crystal structure of dq(Me) involves positional disorder which
precludes detailed structural disc~ssion.~ As representatives of each type of complex,
crystal structure views of compounds a =Cl, rm(Me)CI, dç(Me)*L/iHCl and
6D(Me)Cl are shown in Figures 6.1-6.5, respectively (H atoms are ornitteci for clarity). -
The chelate motif of the ligand is evident in al1 structures except for that of a(Me)CI, in
which the pendant amine is protonated rather than coordinated to the Lewis acidic
bismuth centre. As O bsnvcd for the di thiolate2 and hydroxytholate3 heterocycles,
polymeric packing arrays are made possible by intermolecular Bi--Cl and/or Bi-S
interactions,'" which are distinctively long. E r n e ) adopts a 4: 1 hydrochlonde cluster
array (Figure 6.4) in which the unique chlonde anion acquires a tetragonal site, engaging
four bismuth centers and representing the third Bi-Cl (Bi-Cl) interaction for each
rnolecule of =(Me).
Bis(thio1ate) complexes involving the parent ligand, mNO3 and =Cl, are best
interpreted as ionic matenals composed of the cation da'. on the basis of their relatively
long Bi-O [3.05(2)A] and Bi-Cl p.121(3) A] distances, respectively. These interactions
are responsible for their polymeric lanice arrays, aad the structure of =NO3 only differs
from the hydrated solid _6BN03eH,0Us in that wata adopts one of two anion contacts
- - -- -
Crystal data for =(Me): C,&@N,S,, FW 521 -55, trigonal, space gmup R3 (#146), a = 16.2626(8)& c = 6.579(2)& V = 1506.9(2)A Z = 3.
123 Table 6.1 Selecteâ bond distances (A) for aminoethanethiolates (Bi-CI and Bi-S are
intermolecular contacts).
Figure 6.1 Crystallognphic view of Bi(SCH,CH2NHa, fi.
Figure 6.2 Crystallographic view of Bi(SCH2CH2NH&I =Cl.
Figure 6.3 Cryaallographic view of Bi(SCX,CHJW&Cl m(Me)CI.
Figure 6.4 Crystallographic view of the tetramer of Bi(SCH2CH2NMwl,
K(Me) '/fiCl.
Figure 6.5 Crystallographic view of Bi(SCH2CH2NHMi)Cl, m(Me)CI.
observed in the solvmt fkee structure. In siirprisuig contrast to =Cl, a(Me)Cl has a
substantially shorter (more covalent) Bi-CI interaction [2 -6 1 û(g)A], and is bcst considered
molecular in the solid state aside fiom the intennolecular Bi-S contacts. These
structural differences may be rationalized in ternis of the steric hindrance borne by the
pendant amines in 6&(Me)CI relative to those of the parent ligand. The restricted access
of the amines in m(Me)CI is evident in the Bi-N bond distances m(Me)Cl: 2.84(2)&
2.67(3)A; -NO,: 2.48(2)A; ml: 2.528(9) A, 2.398(8) A], and the comspondingly
weaker auxiliary amine donation in m(Me)Cl enabling a more competitive coordination
of Ci-. The relative withdrawd of the pendant amines in 6B(Me)Cl may be associated
with the distorted cis configuration of the cation moiety, which contrasts the tram
configuration adopted in both -NO, and ml.
The intermolecular interactions (Bi-S) are longest in a enabling an essentially
molecular structure in the solid state, with a distorted pentagonal pyramidal geometry at
bismuth imposed by two cis equatonal sulfbr sites, one apical sulfur site and three
equatorial nitrogen sites, and perhaps irnplicating a stereochernically active lone pair in
the other apical position.
The acyclic structure of rm(Me)Cl contains a six-coordinate, near octahedral
bonding environment for bismuth. A one dimensionai spirocyclic polymeric arrangement
results fiom the association of the bismuth centres by aitemathg chlorine and sui fur
coordinative bridges. The two B i - C i bonds [2.615(4) and 2.636(3)A] are shorter than
the Bi-Clb"@# bonds [2.776(4) and 3.001 (414. Likewise, the Bi-S bond [2.669(3)A]
which is pans to the Bi-Clws is significantly shorter than that which is trons to a Bi-
130 Cl- [2.927(3)A].'" These bond distance cornparisons can be interpreted in terms of
the bismuth center engaging four covalent bonds (tbree chlorine and one sulfùr) (Figure
6.5) and two coordinative bonds (one chlorine and one thioether) h m a neighboring
molecule.
As a demonstration of the potential broad utility of the established synthetic
methods, the antimony analogue (mEC1) of complex -1 has been isolatedb nom an
analogous reaction of aminoethanethiolate with antimony chloride in ethanol and
stnicturally characterized (Figure 6.6). A similar bicyclic arrangement is observed as for
the bismuth complex, but with the complete removal of the chlorine atom fiom the
antimony coordination sphere, giving a rare example of a stibenium cation.
6.3 Conclusions and Future Directions
The homologous series of mono-, bis- and tris- thiolated bismuth complexes
presented above establish the coordinative fiexibility of b i s m u t h o with
aminoethanethiolates and illustrates the ease of stoichiometrically controlling thiolate
coordination chemistry. The pendant amine moieties mediate the high thiophilicity of
bismuth even in the presence of thiolate moieties (raths than thiols) by coordinatively
engaging the bismuth center, so that the stoichiometry of the reaction mixture govems the
degree of thiolation in the isolateci product, thereby overcoming the astoichiornehic
multithiolation, typically encountmd in reactions of bismuth salts with thiols. The
degree of thiolation by the aminoethanethiolate ligand cm be M e r tuned by
manipulating the coordination of the auxiliary amine in two ways: the steric imposition of
Prepared in the Chemîstry 3 101 undergraduate laboratory, Daîhousie University.
Figure 6.6 Crystallographic view of Sb(SCH,CH,NHJCl mC1. Selected bond lmgths
[A]: Bi(1)-S(1) 2.47q6); Bi(1)-S(2) 2.440(6); Bi(1)-N(1) 2.37(2); Bi(1)-N(2)
2.35(2); Bi(1)-Cl(1) 3.577(6).
132 methyl substituents on niîmgen allows for a slightly higher degree of thiolation than the
parent ligand, and the amine can be mtirely uncoupled h m bismuth by protonation, with
retenti on of a mono thiolatobismuth cornplex. These results provide a systematic and
comprehensive series of structuraUy simple thiolatobismuth complexes and the synthetic
approach is Uely applicable to heavy wtals in gend . The potential widespread utility
of the established synthetic methods has been demonstrated in the preparation of an
anthony analogue and the novel bismuth (me&yl~cr)methanethioIates discussed in
Chapter 7.
To date, studies into mixed-thiolate bismuth complexes have not been reported.
Compounds of mixed dithiocarôoxylate ligands have been prepared (Chapter 5.4),
including mixed dithiocarbamate, dithioxanthate, as well a s dithiocarbamate-
dithioxanthate complexes. The controlled thiolation dernonstrateci by the synthesis of the
fmt homologous aminothiolate series suggests a potential for sequential thiolation using
various substituted amine functionaiities:
Ln addition, the aminothiolate ligands could be substitutal for other bihctional thiolate
ligands (e.g. ester-, hydroxy-) to producc mixai functionality compounds:
B is(bihctiona1 thiolate) bismuth sources have been isolated h m aqueous media
[e.g . bismydroxy-/aminothiolato)bismuth nitrates 550/-,] and are potential
intermediates to water stable bismuth carboxylate complexes. One possible reaction
pathway involves Ligand exchange reactioris, such as those employed to prepare
[Bi(SCH,CH20H)S(J (X = CI, Br) 551-52 h m the nitrate salt 550:
OOCR
Also, as bisfiydroxyethanethiolato) bismuth acetate 555 is prepared by recrystallization
of the hydroxythiolate-alkoxythiolate complex 554 h m acetic acid, similar methods may
be emplo yed to prepare other carboxy late analogues:
The high pK,'s and weak chelate abilities of a-amino acids, hydroxycarboxylates
and other simple bifiuictional carboxyIata promote hydrolysis reactions of bismuth in
aqueous media. The above outlined mactions may be expanded and employed to
investigate the structural, spectroscopie and tcaction chemistry of mixed water stable
134 bifunctional carboxylatdthiolate comptexes, incorporating biologically and medicinally
interesting ligands such as glycinate and salicylate:
135 Chapter 7. (Methylester)methinethiolates: The First Ester Complexa of
B i s m u t h o as a Step Toward Modeling ToUoidaI Bismuth Subeltrite'
7.1 Introduction
This chapter descnbes the preparation of the k t ester complexes of bismuthm),
which adopt interrnolecular arrangements maiogous to the ubiquitous dimer structure
observed for citrate complexes of bismuth in CBS 2 û 9 - 1 5 . ~ ' In the absence of
bismuth-ester complexes in the litenhue, section 7.2 introduces the established chemistry
of bismuthtarbonyl compounds. As a backdrop for srnichual discussions, a molecular
orbital mode1 for bismuth complexes is presented in section 7.3.
7.2 Synthesis and Structure of Bismuth-Organocarbonyl Complexes
There are few examples of bismuth compounâs containuig O-carbonyl bound
ligands in the Iiterature, the majonty of which are bihctional and involve ketone and
alkoxide donors. The dipivaloylmethanate compound [Bi(&m),(HdbN] 705 is an
analogue of the ketothiolate [Bi(PhCH {S} CH2C (0)Ph)3 JZICHICIJ 558, which was
discussed in Chapter 5.3. Other sûucturally characterucd compounds include mono- and
polydentate Lewis base adducts. Characterization data is presented in Table 7.1.
Lewis base adducts of bismuth trihalidts are prcpared by direct addition of the
ligand, while bi func tional alkoxides are isolated h m metathesis reactions between bismuth
alkoxides and titanium aikoxides, as well as other cornmon bismuth reactants.
Organobimuth halide adducts (PhBiBr2(dmDia)] and [WBiBr2(dmbir)J have alpo been
prepared and struchrrally charactteruedm
136 Table 7.1 Analytical data for organocarbonyI compounds.
Cornpouad yield X m E s c I R U N M (rxn R p A o o R a V M S
*Svntheses:
7.1) Bi& + n L + Bi&&),
7.2) Bi& + 3 HL + 3 MOH + BiL, + 3 MX + 3 H,O
7.6) BiOJO,), + HL + [Bi(Q(NO,)] + 2 HNO,
7.3) Bi(OR), + HL + Ti(0iQ + Bi(L)(OR'), + Ti(OR)*(OR?, + HOR
7.4) Bi(OR), + HL + Bi(LJ(0Rh + HOR
7.5) BiPh, + 3 HL + BiL, + 3 PhH
The smcture of the cation of the cornplex p i w 6 ] [ B i , I , J 701'~ shows
bismuth in a six coordinate near ocbhedral environment, with al1 six coordination sites
occupied by OBmm ligands p i -O 2.3 lz(8)A; Bi-O-C 1 55.7(8)O]. A bismuth thiolate
&DU adduct [Bi(SC,&),- 5180' has aiso ~CCII structuraîly characterized, and was
discussed in Chapter 5.
701
The monomeric structure of bismuth ethylmaltolate [Bi(emal)J 70P9'
shows a six-coordinate distorted pentagonal bipyrarnidal enWonment for bismuth, with al1
three 0,O '-bidentate Ligands forming five-membered -BiOCCO- rings mi-0- 2.124(7)-
2.250(7)A; Bi-O, 2.420(8)-2.5 1 8(7)A 1. The faciai akoxide oxygen mangement
incorporates the apical site.
702
The aromatic chamcter of the condensed benzene ring of the 4,S-t>enzotropolonato
anion prevents delocalùation of the double bonds in the tropolonate ring (structure
M), allowing the iigand to chelate bismuth in a ketone-alkoxide manner. The bis@#)
complex [Bi@&2(N03)(H20)] 703- shows a six coordinate distortad environment for
bismuth incorporating two 0,O'-tropolonatc ligands [Bi-O, 2.323 and 2.3 1 1 ; Bi-
0- 2.263 and 2.130A~. an O-water molecule [Bi-O 2.621A] and a weakiy coordinated
monodentate nitrate group [Bi-O 2.795Al.
~i,(p-OP~')~(OPf)&f-acac~t]~ 704,'97 a a example of a mixed anionic ligand
cornplex, shows a dimer based onedimcnsionai polyma in the solid state. The six
coordinate bonding environmmt for bismuth is occupied by two pairs of asyrnrnetrically
bridging alkoxide oxygen atoms pi-O 2.19(2) and 2.12(3 ); Bi-O 2.50(2) and 2.69(3)A],
and an ligand [Bi-0- 2.27(3); Bi-& 2.43(4)A 1, forming a six-membered
-BiOCCCO- ring. The i n c d coordination results in very low volatiiity and themal
insbbility of the compound compared to other bismuth dkoxides. Bismuth
tBu acaç
tris(dipivaloyhethanate) (g~ni) pi(dDm)3(HmJ 7 p shows two unique bismuth atoms
each chelated by thm 0.0'- ligands [Bi-O 2.133(7)-2.455(8)A]. A long contact h m a
139 neighbouring molecule pi-O' 3.070(8)A] creates a dimeric structure and gives a seven
coordinate pentagonal bipyramidpl geometry for bismuth. In this case, however, Bi-O and
C-O bond distances do not render an obvious distiaction betwecn the alkoxide and ketone
functionalities in al1 cases.
The trifiinctional OJ,O"-furaldehydohydrazone Lewis base adduct complex
[ s i a 3 C l , ] 706'= [Bi-O- 2.424(8) ; Bi-N 2.654(10); Bi-O* 2.986(9) A] is based on a
faciaily arranged BiCI, unit [Bi- 2.7710); B i C i 2.562(5) and 2.~1q4)Al. A
long chlorine contact pi-CI' 2.909(5)A ] to the w p t y axial site creates a one-dimensionai
polymeric arrangement.
7.3 Secondary Bonding and the tram Effect: the Role of a* Orbitals
The structural features of many bismuth compounds, including the bismuth ester-
thiolates descnbed below, may be rationalized in terms of secondary bismuth bondindm
which warrants a brief defhition. The Lewis ridity and pronounced expansion of the
coordination sphere of bismuth, as well as that of the other heavier p-block elements, was
believed to occur through Iow eacrgy empty dorbitals. Howevcr, calculations suggest
they are too high in mergy to enable significant involvernent in bonding,"' while an
alternative mode1 d s t s the participation of Bi-X a* orbitals. When X is more
140 electronegative than Bi, the antibonding o* orôital will be polarized toward the bismuth
atom:
I
Energy
If this orbital is sufficicntly low in energy it may act as an accepter. The low
electronegativity of bismuth means a higher atomic orbital energy and poorer orbital
overlap with X, resulting in a low energy a* orbital. This model requires a nearly linear
L-Bi-X geometry, and a lengthening of the Bi-X bond as the LBi interaction increases,
due to increased occupation of the a* orbital. This model has been at least qualitatively
usehl in rationalizing the structures of a number of Lewis base adducts of bismuth
phenylbismuth d i h a l i d e ~ , ' ~ ~ ~ as well as the octahedral-bas& structures of Pi(SC,F,),l2-
51 34'6 and the [Bi(SC$,)3(L) J adducts 514-21"' (Chapter 5.2).
7.4 Results and Discussion
Reactions of potassium (methy1ester)methanethiolate with b i s m u t h o chlonde in
95% ethanol at the appropriate stoichiometry give bis[(methylester)methanethiolato]-
bismutho chloride (2: 1) and tris[(me~yle~tcr)rnethanethiolato]bismuth(III)
(3 : 1 ), respectively. Reactions of (methy1ester)methanetbiol with b i s m u t h 0 chloride
also give a which was identified by its distinctive Raman spectnim as the dominant
product, independent of reaction stoichiometry (4: 1,3: 1,2: 1).
14 1 Compowid a adopts a one-dimensional polymeric array in the solid state (Figure
7. l), with hepta-coordination for bismuth imposed by four equatorially disposed sulfur
centers, two oxygen centers (carbonyl) and one chlorine center. The long and essentially
equivalent Bi-S distances mult fiom the strong Pans in.flumcem induced by
intennolecular Bi-S contacts [S(I)-BLS(2a) 154.5(2)' and S(2)-Bi-S(l a) 170.3(1)'].
Although a molecular unit represented by drawing a is indistinguishable in the
polymeric solid state structure, the analogy with the more molecular hydroxy/thio 551'
and amino/thio -)Cl 3*U5us-'89 derivatives is important. The more polymenc structure
of a may be attributed to the restrictions imposed by the backbone sp2 hybridized
carbonyl carbon center and the consequential chelate ring strain.
The structure of the tris(esterthio1ato)biomuth complex a (Figure 7.2) may, at
first glance, be viewed as two trischelated bismuth centers, as observed for the
keto/thio late 5 ~ 8 " ~ and amino thiolate complexes U(R)T9 However, closer inspection
of the Bi-S bond distances [Le. Bi-S(2a). 3.331(2) is substantially longer than Bi-S(2),
2.608(2), Table 7.21 reveals that one of the Ligands clearly functions as an intemuclear
Figure 7.1 Crystallographic view of polym&c ~ r u i g a n m t of [Bi(SCH,COOCH,),C1]
24.
Figure 7.2 Crystallographic view of the dimcric m g c m e n t of [Bi(SCH,COOCH,),)
m.
144
Table 7.2 Cornparison of selected bond lcagths (A) in bismuth-esterthiolate and related
complexes.
CBS
Bi-Cl 3.488(4)
* Average bond distances for two unique molecules.
(&-Bi) bridge, rather than a chelating ligand, imposing a distinct dimer structure m,.
145 In cornparison with the polymeric structure of Z& substitution of the chloride for a third
thiolate is manifested in the dislocation of the . . .S2BiS,Bi.. . chah with consequential
enhancement (shortening) of the three facial thiolate interactions (Table 7.2). The
resulting centrosymmetric dimer mimics the dimenc arrangement evident in citrate
complexes (CBS) 209-15, which is made possible by pendant carboxylate moieties.
0 2 209-15
However, the multiple intemolecular interactions obsenied among dimer units in the
carboxylate complexes are precluded by fornial introduction of the methyl goup to the
carboxylate functionality (to give the ester). The resulting molecular simplicity
highlights the ester fbnctionality as an important stepping Stone to understanding and
controlling the carboxylate chernistry of bismuth.
Preliminary studies have afforded the isolation and structural characterization of a
thiolactate (thiolate-carboxylate) complex of bismuth through similar procedures. The
stoichiometric reaction of BiCI, with thiolactic acid and two equivalents of KOH in
ethanol gave a small crop of crystals of K B i {SCH(CH,)COO}ClJ ZS; (see Figure 7.3).
As with the ester-thiolate complexes, the ligand chelates the bismuth center in an $0-
bidentate manner, however, the carboxylate group also bridges a second bismuth atom in
an 0,O' fashion, giving three coordination contacts for the funetionality. As with
Figure 7.3 Cxystailographic vicw of the polymcric anangcmc1it of
K p i { S C H ( C H ) C Cl] E. Selected bond lmgths [A]: Bi(I )-S(1)
2.5 14(8); Bi(1)-Cl(1) 2.647(8); Bi(l>Cl(2) 2.643(7); Bi(1)-ql) 2.41(2);
Bi(l)-O(1 a) 2.5 l(2); Bi(1)-û(2a) 2.74(2); IC(1)-û(2a) 2.70(2).
147 the thiosalicylate complex 548, intermolecular bonding occun solely through the
carboxylate group, with no long sulfur or chlorine contact.
7.5 Conclusions and Future Direction
Despite the relatively low basicity of the ester (carbonyl) (pK, 21.5; cf. OH p&
16.5, NR, pi&, 9.2. CO; pK, 9.2), the pendant donor intemolecular arrangement
observed for 'colloïdal bismuth subcitrate' has been modeled by anchorhg the Ligand on
bismuth via a thiolate tether. In this way, bifùnctional ligands offer synthetic venatility
to study the interaction of bio-relevant fhctional groups with bismuth, and the hydrolytic
stability of the thiobismuth unit allows for manipulations and observations in aqueous
media.
Additionally, the ester functionality provides a simpler bonding mode1 for the
carboxylate group, which typically chelates bismuth in an 0,O'-manner. In monodenate
carboxylate bonding situations, exocyclic carbonyl oxygen atoms are typically involved
in intermolecular bndging, as observed for lç. bismuth arninocarboxylates (Chapter 4)
and CBS. The introduction of an organic group in the neutral ester huictionality deters
the second (ether) oxygen atom h m possible intra- and intermolecular bonding, and
allows for limited intennolecular coordination.
The amide [C(O)NR,] functionality has the potentiai to accommodate an
intermediate number of intermolecular interactions between those of the carboxy late and
ester complexes. Replacement of a carboxylate oxygen atom with an amine group allows
for both monodentate and N,O-chelating bonding situations, with limited (one)
coordination to the amine hgment. As with ester-thiolate complexes, bifûnctional
148 amide-thiolate ligandsw2 are a rational route to the preparation of bismuth-amide
complexes. Establishing bonding relationships between carboxylate, ester and amide
fiinctionalities is crucial when derivatization of more complex carboxylates are
considered.
The solubilization of bismuth citrate under basic conditions is likely due to
deprotonation of the hydroxy- p u p of the (Hm3- ligand (to fonn the alkoxide) and the
subsequent tridentate chelation of the ligand to thc bismuth center (Chapter 2). Further,
the solubility of the resulting stxucture may be mhanced by the negatively charged
pendant carboxylate group. A comprehensive assessrnent of the role of individual
fùnctional groups of citrïc acid on detmniaing the physical properties of CBS may be
possible through sequential derivatization (structure X: RI, R2, R~ = OMe, NH3,
replacement (structure X: R4 = NHa or removal (cg. malic acid, tricarballylic acid).
Further, and as described in Chaptcr 4, m a s spectrornetry may be employed to study
soluble species.
citric acid X
maiic acid tricarballylic acid
149 The focus of this thesis lies in the interaction of bismuth with organic fiinctional
groups outhed in Chapter 1, howcver, there are several "inorganic" hctionalities which
are comrnonly mcountered in biologicai systenis. The established bihctional ligand
approach may be extended to incorporate highly oxidized main p u p atoms such as
nitrogen (nitrate), phosphorus (phosphate, phosphohate) and sullur (sulfate, Wonate).
nitrate phosphate sulfate
phosphonate sulfonate
The highly acidic nature of these bctionalites pcmiits sufficiently low pH conditions to
deter bismuth hydrolysis reactions and suitable media for simple metathesis teactions in
aqueous media. nie utility of these ligands has been demanstrated by the reaction of
bismuth nitrate and the bihctionai phosphonat~-~arboxylate in water to give
[si(0,PC,H,CO&H20)] 707 or acetone to give the pmtonated
~iH(03PC2H,CO&(H20)] 7 0 8 . ~ Structurai studies of 707 reveals the phosponate
150 functionality bndging three bismuth centers and weakly chelating a fourth. Similar
stnicniral studies may unveil novel bonding situations and intriguing srnichiral
arrangements.
Chapter 8. Experimental
8.1 General Procedures
Melting points wem recordeci on a Fisher-Johns melting point apparatus and are
uncorrected. IR spectta were recorded as Nujol mulls on Cs1 plates using a Nicolet 5 10P
spectrometer. Raman spectra were obtained for powdered and crystalline samples on a
Bniker RFS 100 spcctrometer. Chemicd analyses were perfomed by Canadian
Microanalytical Service Ltd., Delta, British Columbia Solution 'H and "C NMR data
were recorded on a Bruker AC-250 spectrometer. Chernical shifts are reporteci in ppm
relative to and are calibrateci to the intaal solvent signal. Mass spectra were
obtained using a VG Quattro triple quadrupole m a s spectrometer (VG Organic).
Atmosphenc pressure chemical ionkation (APCI) samples were saturated
solutions in 95% ethanol[69. aN0,], acetonitrile [S50-52,555, fi(Me), m(Me)Cl],
dimethyl formamide mC1, =(Me). YiHCl, W e ) ] or dimethylsulfoxide [7A. 7B 1.
Solvent flow [ 1 00% acetonitrile (95% ethanol for 6& 48NOJ at 300pUmin] used a
Shirnadni LC-I OAT liquid chromatograph pump with a Rheodyne syringe loading
sample injector.
8.2 Synthetic Procedures
Bismuth chlonde, bismuth oxychloride, bismuth nitrate pentahydrate, antimony
chloride, 2-aminoethanethi01 hydrochloride, Nfldimethylaminoethanethiol
hydrochloride, methylthioglycolate, glyoxylic acid and thiolactic acid were used as
received fiom Aicirich. Aminoethanethiol (cysteamine) ws used as received h m Fluka.
152 Oxalic acid was used as received h m Fisher. N&,N 'a '-&y lenediwllnetetraaci tic acid
and potassium hydroxide were used as rcceived b m BDH. AU reactions involving
thiols were performed under an atmosphere of N, (to prevent the oxidation of thiols to
disulfides) using standard Schlenk techniques, with the exception of the preparation of
compound m(Me)Cl and Q(Me)Br. Ail compounds are air stable, although 6&Me)CI
changes colour over a perïod of weeks and =Cl is light sensitive. For compound
oD(Me)Br, the dimethylaminoethanethioi hydrobromide sdt is prepand in situ by -
reaction the chloride sait with AgNO, in the appropnate reaction solvent, filtration to
remove AgC1, addition of NaBr and filtration (in the case of the ethanol reaction) to
remove undissolved materials.
The syntheses of [Bi,(~0,)Jm8H20 3& which has been prepared by various
methods, Sb(SCH2CH2NHJC1 mC1 and K p i {SCH(CH,)COO} Cl,] 7C are preiiminary
results and have been attempted only once. Characterization of each is limited to single
crystal X-ray difhction data, which is of poor quality for =Cl. Samples of a contained crystals of varying habit (needles, blocks), not al1 of which were identified.
Thiolate Complexes
The thiolate compounds described below w m prepared by a general procedure,
with the specific conditions for isolation presented in Table 8.1. Between 3 and 10 mm01
of solid bismuth reagent PiCl,, BiBr,, Bi(NO,),.SH,O or SbCl,] was added to a solution
of an aminoethanethiol (parent or dimethyl derivative), an aminoethanethiol
hydrochloride, an aminoethanethiol hydrobromide (generated in situ) or a mixture of an
aminoethanethiol, methylthioglycolate or thiolactic acid with KOH, in 95% ethanol,
153 acetone or wata (150 mL), or glacial acetic acidhvater (6mV14mL). Most reactions are
instantaneous giving yellow solutions (colorless for =Cl), which were stirred ovemight,
filtered and reduced in volume on a rotary evoporator (95% ethanol or acetone) or a hot
water bath (water), until precipitation began. The solution was then re-filtered and cwled
on ice, in the refiigerator (4'C) or h z e r (cO'C), or lefi to evaporate slowly to give
crystalline materials (Table 8.1). Isolateci samples were washed with ethanol, acetone and
ether (25mL each) and dned under vacuum for one hour. Characterization and
spectroscopie data are presented in Tables 8.2-8.4.
Equirnolar reaction mixtures of BiC1, with KSCH,CH,NMe, (7mmo1, prepared in
situ) in 95% ethanol (lSOmL) gave a low solubility powder, which was extracted fkom
the reaction precipitate with dmfand rccrystallizcd by removal of sotvent in vacuo.
Crystals of 6C(Me)* '/JICI were reproducibly Pasteur separated nom a crystalline
mixture and were characterizcd by X-ray crystallography, but data for the bulk sample
were not reproducible. Although the rolubility of compound mr(Me)Cl is very low,
smail samples were crystallized h m aqueous solution and shown to have the same
identity as the bulk reaction mixture prccipitate by a variety of techniques. The bromide
analogue oe(Me)Br was isolated as a powder oniy. Compound a was isolated as a
powder fiom the reaction mixture and rccrystailùed fhm Pmf under vacuum (yellow
needles).
Table 8.1 Reaction and isolation conditions for thiolate complexes.
C o m p o d Reagents, solvents and Crystal Comments amounts (g, mmol) isolation and
pend 6A - BiCl, (1.04,3.35) 4OC, 4 &YS
KOH (1 .88,33.5)
95% ethanol(150 mL)
Ume) BiCI, (2.10,6.64) 4OC, 3 days
KOH (2.24,39.9) 9
95% ethanol(150 mL)
6BNO, Bi(NO,)pSH,O (2.44,s .O3) - ice, 2 hours
HSCH,CH2NH2 (0.78, 1 0)
KOH (0.56, 10)
water (150 mL)
6BNO, Bi(NO,),.SH,O (2.52,5.20 ) - evaporation, light excluded
mH,O HSCH2CH2NH, (1.20, 15.6) 4 days no preconcen tration
KOH (0.875, 15.6) of reaction filtrate
water (1 50 mL)
6BC1 - BiCI, (3.02,9.57) evaporation, light excluded
HSCH2CH2NHpHC1 (326.28.7) 4 days
KOH (3.22,57.4)
95% ethanol(150 mL)
6B(Me)C1 BiCl, (2.09,6.64) - 4OC, 1 day
HSCH2CH2NMe,*HCl (1.88.13.3)
KOH (1 -49.26.6)
acetone (1 50 mL)
155 Table 8.1 Reaction and isolation conditions for thiolate complexes (continued).
Compound Reagents, solvents and Crys ta1 Comments amounts (g, rnmol) isolation and
p e n d
6D(Me)CI BiCl, (2.10,6.64) - precipitation BiCl, dissolved in
1) HSCH,CH,NMepHCI (1.88, 13.3) THF and added
95% ethanol(150 mL), üif(5ûm.L) dropwise to ligand
solution
2) Bi(NO,),.SH,U (2.43, 5.01) precipitation ligand added to
HSCH,CH2NMepHCI(2. 13,lS.O) solution of
water (14 mL)/ acetic acid (6mL) Bi(NO,),eSH,O
bulk sample
isolated as powder
3) crystals h m water wash of evaporation,
reaction mixture precipitate of (2) 12 days
6D(Me)Br BiBr, (2.98,6.64) - d a HSCH,CH,NMep
1) HSCH,CH2NMepHCl (1.89, 13.3) HBr generated in
AgNO, (2.50, 14.7) situ
NaBr (1 .S 1, 14.7)
95% ethanol(l50 mL), thf(5ûmL)
2) Bi(NO,)pSH,O (2.43.5.01) d a HSCH,CH,NMep
HSCH,CH,NMepHCl (2.1 3, 15.0) HBr generated in
AgNO, (3.00,17.7) situ
NaBr (1.82, 17.7)
water (14 mL)/ acetic acid (6mL)
6EC1 - SbC1, (0.91,4.0) <O0C
HSCH,CH,NH,~HC1(1.36,12.0)
KOH (1.36,24.2)
156 Table 8.1 Reaction and isolation conditions for thiolate complexes (continued).
Compound Reagents, solvents and C V ~ Comments amounts (g, mmo1) isolation and
pcriod
7A - BiCI, (1.67,5.28) fiom DMF light excluded
HSCH,COOMe (1.12, 1 0.6) under vacuum
7B - BiC1, (1.65,5.23) 4"C, 1 day
HSCH,COOMe (1.67, 15.7)
KOH (0.88, 16)
95% ethanol(150 mL)
7C - BiCl, (1 .00,3.16) 4OC, 1 day
HSCH(CHJCO0H (0.3Q2.8)
KOH (0.33,S.g)
95% ethanol(1SO mL)
Bismuth Oxulate Octuhydrate ~i&O,) , ].8H20
BiCl, (0.53g, 1.7mmol) and oxalic acid (4.5 1 g, 50.1 mmol) in water (40mL) were
refluxed for 1 1 hours then hot filtered to remove unreacted materiai. Colorless needles of
3A appeared on cooling in air and w m collected &a 2 days. Also prepared by a similar - reaction, replacing BiOCl for BiC1,(1 .mg, 3.84mmol); oxalic acid (3.ûûg, 33.31~101);
water (100mL); reflux period 7 hours; crystallization period 4 &y; crystals remained
under reaction solution until X-ray data collection. Also prepared by a similar reaction,
replacing glyoxylic acid for oxalic acid(Sg, Sx 10-hol); BiCl, (0.5 1 g, 1.6mmol); water
(1 OmL); reflux period 12 hours; crystallization period 6 days; crystals remained under
reaction solution until X-ray data colfection.
Hydrogen Bis(Bismuth Hydrogen A(N.N. N: N'-ethylenediaminetetraacetate) Chlonde
Dihydrate (pi(HEDTA)],H) Cl@2H,O a
BiCl, (1.08g, 3.42mmol) added to ethylenediarninetetraacetic acid (1.00g, 3.42mmol) and
KOH (0.57g, l0mmol) in water ( l50ml) was allowed to stir overnight. The solution was
filtered and concentrated to 40mL over a hot water bath. Colorless needles of a appeared on cooling, collected fier one &y evaporation in air.
Table 8.2 Yields and elemental analyses for dl compounds.
Compound Yield [g, m o l , %] Elernental analysis 1% calc (found)]
6Aow 0.75, 1.4,22 C: 27.63 (27.74) H: 5.80 (5.63)
N: 8.06 (7.99)
6BN03 - 0.48, 1.5,23 C: 1 1.35 (1 1 .40)
H: 2.86 (2.84)
N: 9.93 (9.96)
6BN03*H20 - 0.79,2.4, 35 not determineci
6BC1 - 0.64, 1.6, 17 C: 12.1 1 (12.28)
H: 3.05 (3.00)
N: 7.06 (6.86)
6B(Me)C1 - 0.94,2.1, 3 1 C: 21.22 (21.16) H: 4.45 (4.36)
N: 6.19 (6.04)
159 Table 8.2 Yields and elemental analyses for al1 compounds (continued).
Compound Yield [g, mmol, %] Elmental analysis [% calc (found) J
6D(Me)Cl - 1) 2.72,6.47,97 C: 1 1.42 (1 1.98)
H: 2.62 (2.77)
N: 3.33 (3.42)
2) 1.41,3.35,67 C: 1 1.42(11 .52) FI: 2.62 (2.64)
N: 3.33 (3.32)
3) 0.05, O. 1,2 C: 1 1.42 (1 1.57) H: 2.62 (2.79)
N: 3.33 (3.32)
6D(Me)Br 1) - >95% C: 8.67 (9.19)
H: 2.00 (2.07)
N: 2.53 (2.57)
8.3 Physical and Spectroscopie Data
Table 8.3 Complete vibrational data for al1 compounds.
Compound IR data (cm") Raman data (cm")
4A - 444m, 472w, 496w, 5 MW, 8 ls, 95vs, 136s, 152s, 172s, 204s,
542w, 562w, 592w, 608w, 2281x1, 275w, 293w, 361m, 380x11,
660w, 696w, 770w, 856m, 922s, 407m, 448m, 485m, 581w, 63%,
958m, 9 8 b , 1002w, 1040w, 667w, 71 Sw, 734w, 830w, 920w,
1054w, 1094m, I l lûw, 1170w, 973w, 998w, 1037w, 1 0 5 4 ~ ~ 1098w,
1224w, 1 2 5 4 ~ ~ 1302w, 1318w, 1167w, 1 2 2 5 ~ ~ 125ûm, I302w,
1598s, 1 6 3 4 ~ ~ 1726rn 1324m, 1340w, 1383m, 1437m,
1472m, 1593w, 1629m, 2852w, 291 Os,
2937s, 2958s, 2984m
6A - 290vs, 3 15vs, 4 1 1 s, 487s, 505m, 1 OOvs, 123vs, 177vs, 2 1 1 s, 256m, 286s,
658m, 722w, 82 1 w, 832111, 321s, 663m, 832w, 902w, 944w, 976w,
904w, 940w, 1020w, 1065w, 1021w, 1 0 6 5 ~ ~ 1108w, 1 2 1 0 ~ ~ 1 2 6 7 ~ ~
1 106m, 1208m, 1264w, 1289w, 1298w, 1378w, 1 4 1 9 ~ ~ 1449m,28 18w,
1301w, 1579m,1609w 2849m, 2900s, 29 13s, 2924s, 3 1 53w,
3244m, 3294w
6A(Me) 232w, 266vs, 346m, 415s, 437w, 7ûw, 112s, 162s, 233w, 270vs, 352m, - 522w, 662m, 723w, 762vs, 417w, 437w, 523w, 663m, 764w,
893vs, 95 1 m, 1002s, 1038m, 894w, 953w, 1003w, 1û40w, 1062w,
1060m, 1 0 9 8 ~ . 1 125w, 1 154s, 1 1 2 6 ~ ~ 1 156m, 1218w, 1 2 4 8 ~ ~ 1292m,
121Sm, 1245w, 126Sw, 1291s, 1367w, 1402w, 1432m, 1448m, 1467w,
1 4 0 1 ~ 2 5 7 5 ~ , 2 6 4 8 ~ ~ 27-, 2785~, 2800m7
28 16m, 2850m,29 19s, 2943m, 2980m
16 1 Table 8.3 Complete vibrational data for al1 compounds (continued).
Compound ïR data (cm-') Raman data (cm-')
6BN0, 264vs, 300w, 329m, 469s, 61 8s, 1 14vs, l92m, 216s, 268vs, 282s, 350vs, - 666m, 703w, 723w, 822% 475w, 667w, 712w, 841 w, 92 1 w,
839m, 919m, 968s, 1035s, 1037s, 1066w, 1223w, 1273w, 1381w,
1074m,1221w, 1268w, 13 lgm, 1424w, 1454w, 1572w, 164Sw, 2661w,
1426w, 1573s 2737w, 2828w, 2874m, 291 lm, 2932s,
2948m, 3233w, 3308w
6BCl - 244s, 28 lm, 3 l7s, 330m, 370w, 66vs, 90vs, 106vs, 124vs, 172s, 212vs,
461s, 477m, 589w, 657m,664w, 246vs, 279vs, 322vs, 371vs, 462w,
675w, 722vs, 83 lw, 840w, 591w, 664rn, 83 lw, 845w, 921w,
9 18m, 964s, 101 lm, 1050rn, 963w, 1008w, 1054w, 1081w, 1 103w,
1082m, 1109w, 1155w, 1170w, 1118w, 1214w, 1232w, 1273w, 1289w,
1215w, 1226w, 1275w, 128%. 1372w, 1388w, 1412w, 1426w, 1450w,
1307w, 1412w, 1585w 1587w, 2728w, 2755w, 2830w, 2850m,
2909s, 2919s, 2935m, 2947m, 29561x1,
3098w, 3229w, 3314w
6B(Me)C1 22lvs, 2 9 1 ~ s ~ 358s, 41 ls, 426s, 88m, 103s, 125s, 171m, 21 Ss, 299vs, - 435s, 520s, 661s, 723s, 753vs, 360s, 412w, 438w, 457w, 521w, 664m,
761vs, 894vs, 940s, 951w, 992s, 762w, 895w, 942w, 995w, 1 122w,
1026m, 1039rn, 105ûw, 1097w, 1 160m, 1213w, 1245w, 1297111, 1370w,
1 1 19rn,11 S2m, 1 15%, 1210m, 1403w, 1428m, 1448m, 2723w,
124Srn,l263w, 1291rn,1400w 2787m. 2805m, 2833s, 2869s, 29 1 Os,
2923s, 2953s, 2987m
1 62 Table 8.3 Complete vibrational data for al1 compounds (continued).
Compound IR data (cm-') Raman data (cm-')
6D(Me)Cl 303w, 335m, 41 lw, 5 13w, - 107vs, 127vs, 172s, 220s, 247vs, 334s,
662w, 722m, 756w, 83Sw, 4 12w, 446w, 5 14w, 663m, 757m,
88Sw, 926s, 967w, 101 lm, 885w, 927w, 967w, 101 lw, 1037w,
1035~,1048~,1117w,1149w, 105Ow,12~3w,1229w,1258w,1305w,
1211~,1226~,1256~,1305w, 1365w,1385m,1431m,1451m,
14û4w, 142% 2896w, 2939s, 2955s. 2 9 9 1 ~ 3020m,
3032m
6D(Me)Br S13s, 588m, 658w, 721w, 752w, 75vs, 101m, 1 19vs, 144m, 162vs, - sh, 774s, 834m, 866m,893w, 210vs, 300w, 328s, 408w, 444w, 513m,
922m, 965w, 1 007m, 1 03 1 w, 660m,753m, 878m, 924w, 967w,
1045w, 11 17w, 1 145w, 1 l%Om, 1008w, 1033m, 1045w, 1 117w, 1 147w,
1226w, 1256w, 1321s, 1340~11, 1212w, 1227w, 1257w, 1302w, 1359m,
1425w, 1513vs, 1570vs, 1623vs, 1377rn, 1394w, 1427m, 1451m,
1639w, 3402vs 1464w, 147Sw, 284 1 w, 2893w, 2932w,
2947s, 2960s, 2983w, 302ûm, 3074w
6BNO, 258vs, 285vs, 347m, 481s, - 86vs, 1 17s,153w, 187m, 2 1 Os, 268vs,
eH,O 662m, 688w, 722w, 823s, 839111, 287vs, 359vs, 478w, 665w, 713w,
921 m, 966m, 1045s, 1 082m, 8 4 h , 922w, 96 1 w, 1 û45s, 1 076w,
1 1 12w, 1223s, 1 4 2 5 ~ s ~ 1602s, 1 1 12w, 1222w, 128ûw, 1294w, l338w,
1636s, 175Sw 1385w, 1423w, 1451 w, 1598w, 2744w,
2860w, 2924m, 2964w, 3 154w, 3237w,
3297w
7A - 555w, 681w, 770w, 874s, 886w, 95vs, 1 17s,sh, 147s, 187s, 227vs,
986m, 994m, 1 ldlm, 1206m, 260vs, 350m, 399w, 561w, 686w,
1296m, 13 18m, 1676s, 1 707s 768w, 888m, 984w, 1 M W , 1204w,
1325w, 1376w, 1392w, 1428w, 1673w,
2903s, 2940m, 2959rn,3044w
163 Table 8.3 Complete vibrational data for dl compounds (continued).
Compound IR data (cm-') Raman data (cm-')
7B - 569m, 583m, 681 w, 71 lm, 95vs, 146m, 195m, 22 lm, 266vs,
772w, 864m, 88Uw, 889m, 292vs, 334m, 402w, 580w, 714w,
899w, 90%, 992s, 1 OZlw, 769w, 885w, 908w, 990w, 1 1 5 l w,
1141m,1204s, 1287~~ 1308s, 11 81w, I296w, 1397w, 1435w, 1696w,
1397m, 1434s, 1558w, 1579w, 2886s, 2956m, 2976m, 2988m, 3034w
1605w, 1623w, 1691m,173Srn
1 64 Table 8.4 Melting points, prominent APCI-MS peaks, and 'H and "C NMR data for al1
cornPound mp NMR ( D ~ s 0 - d ~ " APCI-MS
(Oc) ' H 13C [Cone Voltage: m/z (% rd . intensity) J
4~ [2971 - - - - 6A - 87 2.24,3.00, 31.0, SV: 209(100), 361(48)
3.57 47.6 30V: 209(24), 36 l(100)
6A(Me) 140 2.31,2.80, 25.3, SV: 209(1ûû), 417(7) 3.53 44.9, 30V: 209(23), 41 7(100)
65.8
6BNO, - 11581 3.78,3.96, 30.3, SV: 361(100) 4.13 49.1
6BN0, - - - w 3 1 ref Us
*H,O
6 x 1 - 11911 3.77,3.96 30.3, 10V: 209(89), 320(54), 393(100)
49.0 30V:284(75),320(100),393(7)
6B(Me)C1 [125] 2.76,3.50, 26.1, SV: 209(100), 417(2), 453(2) - 4.32 44.9, 30V: 209(25), 348(100), 41 7(5 l),
66.9 453(2)
6D(Me)Cl [205] 2.77.3.30, 23.2. 10V: 2O9(l OO), 348(79), 384(9), 41 7(4), - 4.98,9.02 42.7, 421(57), 453(4)
60.8 30V: 209(10), 348(100), 384(4),
4 1 7(3)
* Decomposition occurs over a broad range and the temperature given represents the
onset of blackening.
** Signals are generally poody resolved.
165 Table 8.4 Melting points, prominent APCI-MS pcaks, and 'H and "C NMR data for al1
cornpounds (continued).
Compound mp NMR (DMsO-d~" APCI-MS [dpl' (OC) 'H "C [Cone Voltage: m/z (% rel. intensity)]
175.8
* Decomposition occurs over a broad range and the temperature givm repments the
onset of blackening.
** Signals are generaily poorly resolved.
166 Table 8.5 Peak assignments of the APCl mass spectra of bis(hydroxyethanethîo1ato)-
bismuth sale [Bi(SCH,CH,OH)&'J.
X cone voltage 1 OV cone voltage 30V
m/z (%) assignment m/z (%) assignrnent
NO, 285 (9) [-BiSqH40-J+ 241 (3) [Bis]'
Table 8.6 M S M assignments for bis(hydrOxyethanethioIato)bimuth(III) salts
Daughters cone m/z (%) of(dz) vo l tage0
- --
NO, 326 10 209 (18) Bi'
550 241 (78) [BIS]'
285 (100) [-BiSC,H40-1'
326 (32) [-BiSC,H,O-+NCCH,]'
NO3 363 10 209 (22) Bi'
550 241 (43) [Bis]'
CI 321 10 209 (28) Bi'
Cl 362 10 209 (12) Bi' -
241 (45) [BIS]'
285 (100) [-BiSC,H,O-]'
321 (48) FI-SC2H40H]+
361 (26) mOC2H4SBiCl + NCCH,]'
8.4 X-ray Crystallography Data
Table 8.7 Crystallographic data for dl complexes.
- -
empirical formula C,H,&O, c,0&2iC1,SO&09
Formula Weight 826.14 534.45
crystaI description yellow, needle colorless, needIe -
crystal system triclinic rnonoclinic
space group P-1 (#2) CUc (#Ils)
a CA) 9.370(3) 25.203(6)
b (4 1 1.106(3) 8.979(4)
Z value 2 8
Qak W m 3 ) 3.180 2.453
R; k 0.03 7; 0.040 0.036; 0.040
Goodness of Fit 1.44 1.64 Indicator
Table 8.7 Cxystallographic data for compounds (continued).
a mBNQ 6Bc1 empirical formula C a , ,BiN3S3 C4H&i%0,S2 C,H,,BiCN2S,
Formula Weight 437.39 423.26 396.71
crystal description yellow, needle needles light yellow, needle
crystal system monoc h i c trigona1 triclinic
space group P2,h (M4) P3,21 (#152) P-1 (#2)
a (4 5.69(1) 8.933 1(10) 8.747(2)
b (4 11.614(9) 8.933 l(10) 9.63 6(2)
C (4 19.562(3) 12.156(4) S.98Cyl)
Z value 4 4 2
O& Wcm3) 2.249 2.5 10 2.67 1
R; ka 0.043; 0.050 0.037; 0.045
RI; ~ l 3 . 2 ~ 0.0669; O. 1526 ~I-OJ
RI; wIUb 0.0683; 01527 (ail data)
Goodness of Fit 1.23 5.157 1 .O7 Indicator
170 Table 8.7 Crystallographic data for al1 compoimds (contiaud).
Formula Weight 452.81 393.19 420.54 --
crystal description long yellow, blocks yeiiow, square- plate needle-like
crystal system monoclinic teiragona1 monoclinic
space group pz1 (#4) 1-4 (#82) P2,k (#14)
a (A) 8. 122(3) 1 5.082(5) 6.850(2)
b (4 1 O, 1 07(2) 1 5 .082(5) 1 3.977(2)
Z value 2 8 4
Goodness of Fit 1.14 2.8 1 4.3 1 Indicator
Table 8.7 Crystallographic data for ail compounb (continued).
=ci* 7A empirical formula C,H,,CN2S2Sb C&,BiClO,S,
Formula Weight 309.48 454.70
crystal description colorless, needlc light yellow, needle
crystal system rnonoclinic monoclinic - space group P 2 , h (#14) Pa (#7)
a (A) 5866(2) 8.092(2)
Z value 8 2
Qd. (%cm3) 3.13 1 2.579
R; R, 0.082; 0.080 0.036; 0.027
Goodness of Fit 4.94 1.57 Indicator
172 Table 8.7 Crystallographic data for dl wmplexcs (continued).
28 x empirical formula C&l,,BiO,S, C,H,BiCl,KO,S
Formula Weight 524.36 423.1 1
crystal description yellow, needle colorless, needle
crystal system triclinic monoclinic
space group P-1 (#2) P2,k (# 1 4)
Z value 2 4
Goodness of Fit 1.60 1.18 Indicator
* Prelirninary structure.
a R = ~ll~ol- I F C ~ ~ I CIFOI; = [ Z W ( ~ O ~ - I F C ~ ) ~ 1 ZWFO~I
2 2 K RI = CI(Fo1- (Fc(l/ ZIFo(; wR2 = {C[W(F~-FC~)~] 1 Z[w(Fo ) 1)
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